THERMODYNAMICS
Some Important common thermodynamic terms
1. System :
The part of the universe selected for thermodynamic study is called system. For example boiling of water in a beaker.
2. Surroundings :
The remaining part of the Universe around the system, which is not under study, is called surroundings. For example, boiling of water in a beaker is an example of system and everything else around the beaker is the surroundings.
3. Types of System :
Generally system may be classified into three categories:
(i) Open system: A system, which can exchange matter as well as energy with its surroundings, is called an open system. For example, boiling of water in an open beaker.
(ii) Closed System: A system, which may exchange energy but not matter with surroundings, is called a closed system. For example, system remains inside the vessel.
(iii) Isolated system: A system which can neither exchange matter nor energy with the surroundings is called an isolated system.
4. Homogeneous and Heterogeneous System :
(i) Homogeneous system: A system is said to be homogeneous if it is uniform throughout. Such type of system consists of only one phase. For example, a system containing only a pure solid or a pure liquid or a pure gas or completely miscible liquids or gases etc.
(ii) Heterogeneous system. A system is said to be heterogeneous if it is not uniform throughout. Such type of system consists more than one phase i.e., Polyphase. For example, a system containing a mixture of two immiscible liquids or gases or solids etc.
5. Thermodynamic Properties:
(i) Extensive property, and (ii) Intensive Property.
(i) Extensive property:
The properties, which depend on the amount of the material in the system, are called ‘Extensive properties’. For example, volume, internal energy, heat capacity, free energy, mass heat content, entropy, etc.
(ii) Intensive property:
The Properties, which do not depend (independent) on the amount of the material but depend upon the nature of the material in the system, are called intensive properties. For example, viscosity, surface tension, thermal conductivity, boiling point, freezing points, refractive index, Vapour pressure of as liquid, temperature, density, specific heat etc.
6. Thermodynamic Equilibrium
(i) Thermal Equilibrium.
(ii) Mechanical equilibrium.
(iii) Chemical equilibrium.
(i) Thermal Equilibrium: A system is said to be in thermal equilibrium if there is no flow of heat from one portion of the macroscopic system to the another portion. This is possible only if the temperature remains the same throughout in all parts of the system.
(ii) Mechanical Equilibrium: A system is said to be in mechanical equilibrium if no mechanical work is done by one part of the macroscopic system to the another part of the system. This is possible only if the pressure remains constant throughout in all parts of the system.
(iii) Chemical Equilibrium: A system is said to be in Chemical equilibrium if the composition of the various phases in the system does not change with time.
7. Thermodynamic Process
It is the operation, which brings about the changes in the state or system. It is of the following types:
(i) Isothermal Process(dT=0)
(ii) Adiabatic Process(dq=0)
(iii) Isobaric process(dp=0)
(iv) Isochoric process(dv=0)
(v) Cyclic process(dE=0)
Path function: It is the property whose change depends upon the path followed by it and not upon the initial & final state of the system.eg. work
State function: It is the property whose change depends upon the initial & final state of the system and not upon the path followed by it
(i) Reversible process: A process is said to be reversible if it is carried out infinitesimally slowly so that the driving force is only infinitesimally greater than the opposing force. Such types of processes are ideal and cannot be realized in practice. This is because a reversible process requires infinite time for its completion.
(ii) Irreversible process: A process is said to be irreversible if it is not carried out infinitesimally slowly but the change is produced rapidly so that the system slowly does not remain in equilibrium condition. Both the reversible and irreversible process may be understood as follow.
LAWS OF THERMODYNAMICS
1. First Law is simply known as the ‘Law of conservation of energy’. The law may be stated in any one of the following ways:
(i) Energy can neither be created nor destroyed by any physical or chemical change. However, it can be changed into equivalent amount of the other form.
(ii) The total energy of isolated system remains constant.
(iii) It is impossible to construct a perpetual motion machine i.e., a machine, which works without consuming energy.
(iv) The total sum of mass and energy is constant in the Universe though these are interconvertible consuming and are related to each other by the expression
(E=mc2)
`
Where E = energy produced by destruction of mass ‘m’
c = velocity of light.
Therefore, the first law is modified and stated as “The total mass and energy of an isolated system remains unchanged”.
Mathematical Formulation
Let us consider a system having internal energy E1 in a particular set of condition. Suppose the q amount of the heat supplied to the system. Supplying the heat increases the internal energy of the system. Let the internal energy of the system in the final state is E2 and work done on the system is w, then:
E2 = E1 + q + w or E2-E1 = q + w or ΔE = q + w ------- (1)
Here ΔE = change in internal energy
Limitations
(i) It is unable to explain why do the physical and chemical processes occur in a natural direction. For example, ice melts at room temperature but water does not freeze at room temperature.
(ii) It does not predict the feasibility of a process in a particular direction.
(iii) It does not put any restriction on the direction of flow or heat. For example, without any external aid, ice may be used to heat water by extracting heat from ice at lower temperature and supplying it to the water at higher temperature.
(iv) It does not tell about the extent of convertibility of one form of energy into another. Due to the above limitations second law of thermodynamics came into existence.
Second Law of Thermodynamics
It may be stated in following ways:
(i) Heat cannot be completely converted into work without leaving changes either in the system or in the surroundings.
(ii) It is impossible for a self-acting machine, unaided by any external agency; to convey heat from a body at a lower temperature to one at higher temperature i.e., heat cannot pass from a colder body to a warmer body. Some work must be expanded to achieve this.(R. Clausius statement)
(iii) It is impossible for a cyclic process to take heat from a cold reservoir and convert it into work without at the same time transferring heat from a hot to a cold reservoir.(Kelvin statement)
(iv) All spontaneous processes or naturally occurring processes are thermodynamically irreversible; therefore, the entropy of the Universe is increasing continuously.
(v) The entropy of the Universe remains constant in a reversible process but it increases in an irreversible process.
ENTROPY:
The term ‘entropy’ is introduced by R.J.E.Clausius. Entropy is a Greek word (‘trope’ means change and ‘en’ stands for energy). Entropy is the property of substance, which measures the disorder or randomness in a system and is represented by ‘S’. Entropy is larger in case of more randomness. It is also a measure of the unavailable energy. In general for any substance
SVapour >SLiquid >SSolid
ΔS = qrev / T
Units:
Entropy change is expressed by a heat term divided by the absolute temperature.
In S.I. units entropy is expressed in JK-1 mol-1 (1 cal=4.186J)
Physical Significance
(i) Entropy is a state function: It does not depend upon the path by which the change takes place.
(ii) Entropy is a measure of randomness (disorder) of the system. Greater the randomness, higher is the entropy of the system.
SGas > SLiquid > SSolid
ENTROPY CHANGES FOR AN IDEAL GAS
Since entropy is a state function of system. Its value for a pure substance depends upon any two of the three variables P, T and V. Since temperature (T) is considered generally as one of the variables, the second variables to be considered may be either P or V.
To derive ideal gas equation for entropy change is considered over following cases:
Case I: Temperature (T) and volume (V) variations
Case II: Temperature (T) and Pressure (P) variations
CaseI: consider an ideal gas having volume V at temperature T and pressure P. Let the system absorbs an infinitesimally small amount of heat dqrev reversibly at temp. T, then the entropy of the system increases.
dE = dq –dW (1st law of thermodynamics) ------------------(1)
dE = CvdT ------------------(2)
dq = TdS ---------------(3)
dW = -PdV -------------(4)
Using (1),(2),(3) & (4) we have:
dS = CvdT / T + RdV / V
On integrating above equ. within limits S1 to S2, T1 to T2 and V1 to V2.
ΔS =nCV ln T2/T1 + nR ln V2/V1 for n moles of an ideal gas. --------------- (5)
Case II:
P1V1 / T1 = P2V2 / T2 ------------------ (6)
Cp –Cv = R ---------------- (7)
From (5), (6) & (7) we have:
ΔS= CP ln T2/T1 - R ln P2/P1
Special cases:
Isothermal Process: ΔST = R ln V2/V1 or - R ln P2/P1
Isobaric Process: ΔSP = CP ln T2/T1
Isochoric Process: ΔSV = CV ln T2/T1
Entropy Change in Reversible and Irreversible Process
Entropy change for a reversible process is always zero i.e. ΔSTotal = 0 and the entropy change for an irreversible process is always +ve. i.e. there is no net change in entropy for a reversible process and entropy always increases in an irreversible process.
Physical significance of work function
Decrease in change in work function (Helmholtz free energy function) is equal to max. work obtained from the system during change i.e. –ΔA = Wrev. = Wmax.
Physical significance of Gibb’s free energy
Decrease in change in free energy is equal to max. work other than pressure- volume work that can be obtained from the system during change i.e. –ΔG = Wrev. - P ΔV.
Gibb’s Helmholtz Equation in terms of free energy:
G = H-TS (1)
∆G = ∆H - T∆S (2)
Also dG = VdP- SdT (3)
(∂G / ∂T)p = -S (4)
from equ. 1& 4
G = H + T (∂G / ∂T)p
Also, - ∆S = S1 – S2
= [∂(G2-G1) / ∂T]p (from equ. 4 )
= [∂(∆G ) / ∂T]p (5)
from equ. 2 & 5
∆G = ∆H + T [∂ (∆G) / ∂T]p (6)
Gibb’s Helmholtz Equation in terms of work function (Helmholtz function):
A = E-TS (1)
∆A = ∆E - T∆S (2)
Also dA = PdV- SdT (3)
(∂A / ∂T)v = -S (4)
from equ. 1& 4
A = E + T (∂A / ∂T)v
Also, - ∆S = S1 – S2
= [∂(A2-A1) / ∂T]v (from equ. 4 )
= [∂(∆A ) / ∂T]v (5)
from equ. 2 & 5
∆A = ∆E + T [∂ (∆A) / ∂T]v
Alternative form of equ. (6)
[∂ / ∂T(∆G / T)]p = - ∆H / T2 (on differentiating ∆G / T w.r.t. T at constant P)
Significance:
1) Idea of spontaneity of a reaction
∆G < 0 reaction will be non spontaneous.
∆G > 0 reaction will be spontaneous.
∆G = 0 reaction will be in equilibrium.
Since ∆G = ∆H - T∆S
Consider exothermic & endothermic reactions for both +ve & -ve values of ∆H & ∆S with increase and decrease of temperature.
2) In the study of Galvanic cells as:
nFE = - ∆H + TnF[(∂E / ∂T)p (as ∆G = -nFEcell for an electrical cell)
Chemical Potential (Partial molal / Molar free energy)
It is defined as the change in free energy of the system when 1 mole of that particular substance is added at constant temp. & pressure, to such a large quantity of the system so that there is no appreciable change in overall composition of the system.
μi = (∂G / ∂ni)T,P,n1,n2----------
Clausis – Clapeyron Equation:
Consider 1 mole of a substance in two phases A & B in equilibrium at constant Temp & Pressure.
For this,
∆G = 0 or GB – GA = 0 (1)
For small change in pressure as P+dP, temperature as T+dT
Relative change in Gibb’s free energy for the two phases is as;
For phase A, GA+dGA & for phase B, GB+dGB
For such a small change, the system is still considered to be in equilibrium, so
GA+dGA = GB+dGB (2)
From (1) & (2)
dGA = dGB (3)
Also, dG = VdP-SdT (4)
From (3) & (4)
dP / dT = SB-SA / VB-VA = ∆S / ∆V
Also, ∆S = q / T
So dP / dT = q / T ( VB-VA )
For liquid – vapour equilibrium,
dP / dT = ∆HV / T( Vg-Vl ) (5)
∆HV = molar heat of vaporization.
Similarly for solid – liquid & solid –vapour equilibrium.
Integrated form of Clausis – Clapeyron Equation:
In comparison to gas (Vg), the Vs & Vl may be neglected and hence
Vg-Vs = Vg
Vg-Vl = Vg
Now equ. (5) may be written as,
dP / dT = ∆HV / T Vg
(6)
If vapours are assumed to behave ideally then,
Vg = RT / P
(7)
From (6) & (7)
dP / P = (∆H / RT2) dT
(8)
Assuming ∆H remains constant(condition for integration) & then integrating the above equ. Within limits P1 to P2 & T1 to T2 we have;
2.303 log P2 / P1 = ∆H / R [T2-T1 / T1T2] (9)
Applications:
1) Determination of molar heat of vaporization.
2) Determination of boiling points of a liquid at different pressures.
3) Determination of vapour pressures of a liquid at different temperatures.
Numericals:
1) Calculate the change in entropy for 1 mole of an ideal gas when its temperature rise from 300K to 600K under i) Isochoric condition & ii) Isobaric condition. (Cv = 2.5R)
Soln: T1 = 300K T2 = 600K n = 1
ΔS= CP ln T2/T1 - R ln P2/P1
ΔSV = nCV ln T2/T1 + nR ln V2/V1
For Isochoric condition
Using ΔS = nCV ln T2/T1 ΔS = 14.40J/K/mole
For Isobaric condition
Using ΔS = nCp ln T2/T1 & Cp –Cv = R ΔS = 20.16J/K/mole
2) The energy change (ΔG) in a process are found to be -138KJ at 303K & -135KJ at 313K. Calculate the enthalpy change at 308K.
Soln:
ΔG at (303 +313/2) K = -138-135/2
ΔG at308K = -273/2
= -136.5KJ
[∂ (∆G) / ∂T] = ΔG at 313 - ΔG at 303/T2 – T1
= -135 + 138/10
Now using ∆G = ∆H + T [∂ (∆G) / ∂T]p
∆H = - 228.9KJ
3) Calculate the change in volume for melting of 1 gm. mole of phenol. Given latent heat of fusion = 3250 cal/gmole.Melting point of phenol = 330K dP/dT = 287atm./K
Soln:
Using dP / dT = ∆HV / T( Vl-Vs )
( Vl-Vs ) = 0.034 ml
4) The latent heat of vaporization of water is 540 cal/gm at 1000C. Calculate the pressure at which water must be heated to produce superheated steam at 1500C.
Soln:
∆Hvap. = 540cal/gm
= 540 Χ 18 cal/mole
T1 = 1000C = 373K T2 = 1500C = 423K
P1 = 1 atm. P2 = ?
Now using 2.303 log P2 / P1 = ∆H / R [T2-T1 / T1T2]
P2 = 4.71 atm.
Thursday, July 31, 2008
Assignment-4
Assignment-4
1. What is Lambert’s Law?
2. What is Lambert-Beer Law?
3. Define absorbance and transmittance of a solution.
4. Describe briefly the process which takes place when the solution of a metallic salt is sprayed into a flame?
5. Name the important components of a flame –photometer.
6. Write short notes on the following:
(i) Oileness (ii) Neutralization number (iii) Saponification number
(iv) Cloud point and pour point of lubricant.(iv) Synthetic lubricants
7. Define Viscosity Index. How is it determined for a lubricant?
8. Why graphite and MoS2 preffered as solid lubricants?
9. What do you understand by wear ? Give precise definition.
10. What is friction and what are its consequences?
11. Give a brief account of the classical laws of frictions
12. Give the Principle and Applications of I.R.& U.V. spectroscopy.
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1. What is Lambert’s Law?
2. What is Lambert-Beer Law?
3. Define absorbance and transmittance of a solution.
4. Describe briefly the process which takes place when the solution of a metallic salt is sprayed into a flame?
5. Name the important components of a flame –photometer.
6. Write short notes on the following:
(i) Oileness (ii) Neutralization number (iii) Saponification number
(iv) Cloud point and pour point of lubricant.(iv) Synthetic lubricants
7. Define Viscosity Index. How is it determined for a lubricant?
8. Why graphite and MoS2 preffered as solid lubricants?
9. What do you understand by wear ? Give precise definition.
10. What is friction and what are its consequences?
11. Give a brief account of the classical laws of frictions
12. Give the Principle and Applications of I.R.& U.V. spectroscopy.
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Assignment-3
Assignment- 3
1. What are the differences between Galvanic cell and Electrolytic cell?
2. What is Galvanic series?
3. What do you mean by corrosion? How does it differ from erosion?
4. Explain how corrosion can be controlled by proper designing?
5. What are the effects of temperature, pH, over voltage and reactivities of metals influences the corrosion?
6. Write preparation properties and applications of following polymers
(a) Polyvinyl Chloride (PVC) (b) Polyvinyl acetate (PVA)
(c) Bakelite (d) Urea formaldehyde (UF) (e) Styrene rubber (GR-S / Buna-S / SBR)
(f) Nitrile rubber (GR-N / Buna-N / NBR) (g) Butyl rubber (GR-I)
7. What do you understand by crystallinity of a polymer?
8. What is the difference between thermosets and thermoplastics? Give their charcterisics and suitable examples.
9. Explain the addition and condensation polymerization reactions with one example for each.
10. What do you understand by Co-ordination Polymerisation? Explain with example.
1. What are the differences between Galvanic cell and Electrolytic cell?
2. What is Galvanic series?
3. What do you mean by corrosion? How does it differ from erosion?
4. Explain how corrosion can be controlled by proper designing?
5. What are the effects of temperature, pH, over voltage and reactivities of metals influences the corrosion?
6. Write preparation properties and applications of following polymers
(a) Polyvinyl Chloride (PVC) (b) Polyvinyl acetate (PVA)
(c) Bakelite (d) Urea formaldehyde (UF) (e) Styrene rubber (GR-S / Buna-S / SBR)
(f) Nitrile rubber (GR-N / Buna-N / NBR) (g) Butyl rubber (GR-I)
7. What do you understand by crystallinity of a polymer?
8. What is the difference between thermosets and thermoplastics? Give their charcterisics and suitable examples.
9. Explain the addition and condensation polymerization reactions with one example for each.
10. What do you understand by Co-ordination Polymerisation? Explain with example.
Assignment-2
Assignment- 2
100 ml. of a sample of hard water neutralizes exactly 12 ml. of 0.12 N HCl using methyl orange as indicator. What kind of hardness is present? Express the same in terms of an equivalent of CaCO3.
2. 100 ml. of a water sample required 12.4 ml. of N/50 H2SO4 for neutralization to phenolphthalein end point. Another 15.2 ml. of same acid was needed for further titration to methyl orange end point. Determine the type and amount of alkalinity.
50 ml. of water sample requires 10 ml. of 0.01 N EDTA when titrated using buffer solution (pH=10) to attain the end point. Calculate the total hardness of a sample in terms of ppm equivalent of CaCO3 per litre.
4. 200ml. of hard water sample require 30 ml. of 0.02 M EDTA with NH4 Cl-NH4OH buffer and EBT indicator. Another 200 ml. of the sample is boiled for about half an hour and after filtering the ppt. the volume of filtrate is made 200 ml. again by the addition of distilled water.20 ml. of this boiled water sample requires 5 ml. of 0.01 ml. EDTA following the same procedure. Calculate the temporary and permanent hardness of the sample.
5. A water sample on analysis gives the following data : Ca2+ = 20 ppm, Mg2+ = 25 ppm, CO2 = 30 ppm, HCO3- = 150 ppm, K+ = 10 ppm. Calculate the lime(87%pure) and soda (91% pure) required to soften 1 million litres of water sample.
6. Calculate the quantity of lime and soda required for softening 60000 liters of water containing CO2 = 20mg/L, Ca(HCO3)2 = 20 mg/L, Mg(HCO3)2 = 25mg/L, HCl= 8.4 mg/L, Al2(SO4)3 = 40mg/L and Mg Cl2 = 12 mg/L.
7. What is the principal involved in reverse osmosis process of desalination of water? Describe the process and its advantages.
8. What is Electro dialysis and how is it carried out? Discuss the process, its advantage and limitations.
100 ml. of a sample of hard water neutralizes exactly 12 ml. of 0.12 N HCl using methyl orange as indicator. What kind of hardness is present? Express the same in terms of an equivalent of CaCO3.
2. 100 ml. of a water sample required 12.4 ml. of N/50 H2SO4 for neutralization to phenolphthalein end point. Another 15.2 ml. of same acid was needed for further titration to methyl orange end point. Determine the type and amount of alkalinity.
50 ml. of water sample requires 10 ml. of 0.01 N EDTA when titrated using buffer solution (pH=10) to attain the end point. Calculate the total hardness of a sample in terms of ppm equivalent of CaCO3 per litre.
4. 200ml. of hard water sample require 30 ml. of 0.02 M EDTA with NH4 Cl-NH4OH buffer and EBT indicator. Another 200 ml. of the sample is boiled for about half an hour and after filtering the ppt. the volume of filtrate is made 200 ml. again by the addition of distilled water.20 ml. of this boiled water sample requires 5 ml. of 0.01 ml. EDTA following the same procedure. Calculate the temporary and permanent hardness of the sample.
5. A water sample on analysis gives the following data : Ca2+ = 20 ppm, Mg2+ = 25 ppm, CO2 = 30 ppm, HCO3- = 150 ppm, K+ = 10 ppm. Calculate the lime(87%pure) and soda (91% pure) required to soften 1 million litres of water sample.
6. Calculate the quantity of lime and soda required for softening 60000 liters of water containing CO2 = 20mg/L, Ca(HCO3)2 = 20 mg/L, Mg(HCO3)2 = 25mg/L, HCl= 8.4 mg/L, Al2(SO4)3 = 40mg/L and Mg Cl2 = 12 mg/L.
7. What is the principal involved in reverse osmosis process of desalination of water? Describe the process and its advantages.
8. What is Electro dialysis and how is it carried out? Discuss the process, its advantage and limitations.
Assignment-1
Assignment-1
1. Define Thermodynamics and mention its scope. State and explain the important laws of thermodynamics. What are its limitations?
2. State and explain the first law of thermodynamics. Derive a mathematical formulation of the law. Justify the law on the basis of some common observations and discuss its limitation.
3. Five moles of an ideal gas expand isothermally and reversibly at 27 C from an initially volume of 5dm to 50 dm against a pressure that is greatly reduced. Calculate G & S for the process. (R= 8.314 J/K/mol)
4. Calculate the change in entropy for one mole an ideal gas when its temperature rises from 300k to 600k (i) Isochoric condition (ii) Isobaric condition
Cv = 2.5R
5. Water boils at 373 K at one atmospheric pressure. At what temperature will it boil when atmospheric pressure becomes 528 mm of Hg at some space station? Latent heat of water = 2.28KJ/g
6. At 373.6 K and 372.6 K the vapour pressure of water are 1.018 and o.982 atm. resp. Calculate the heat of vaporization of water.
7. The free energy change ( G) accompanying a given process is – 85.77 and -83.68 kj at 25 C and 35 C respectively. Calculate the change in enthalpy for the process at 30 C.
8. Calculate the number of phases in the following:
(a) SR SM
(b) I2 (s) I2 (g)
(c) MgCO3(s) MgO(s) + CO2 (g)
(d) N2O4 (g) 2NO2(g)
9. How many degrees of Freedom are present in the following system?
a) A gas in equilibrium with its solution in a liquid
b) Two partially miscible liquids in the absence of vapour
10. What do you understand by condensed system.
1. Define Thermodynamics and mention its scope. State and explain the important laws of thermodynamics. What are its limitations?
2. State and explain the first law of thermodynamics. Derive a mathematical formulation of the law. Justify the law on the basis of some common observations and discuss its limitation.
3. Five moles of an ideal gas expand isothermally and reversibly at 27 C from an initially volume of 5dm to 50 dm against a pressure that is greatly reduced. Calculate G & S for the process. (R= 8.314 J/K/mol)
4. Calculate the change in entropy for one mole an ideal gas when its temperature rises from 300k to 600k (i) Isochoric condition (ii) Isobaric condition
Cv = 2.5R
5. Water boils at 373 K at one atmospheric pressure. At what temperature will it boil when atmospheric pressure becomes 528 mm of Hg at some space station? Latent heat of water = 2.28KJ/g
6. At 373.6 K and 372.6 K the vapour pressure of water are 1.018 and o.982 atm. resp. Calculate the heat of vaporization of water.
7. The free energy change ( G) accompanying a given process is – 85.77 and -83.68 kj at 25 C and 35 C respectively. Calculate the change in enthalpy for the process at 30 C.
8. Calculate the number of phases in the following:
(a) SR SM
(b) I2 (s) I2 (g)
(c) MgCO3(s) MgO(s) + CO2 (g)
(d) N2O4 (g) 2NO2(g)
9. How many degrees of Freedom are present in the following system?
a) A gas in equilibrium with its solution in a liquid
b) Two partially miscible liquids in the absence of vapour
10. What do you understand by condensed system.
Tutorial-8
TUTE SHEET-8
ANALYTICAL METHODS
1. What is Thermogravimetric analysis? Describe briefly.
2. What do you understand by a thermogram and a differential thermogram?
3. What do you understand by hypsochromic shift and bathochromic shift?
4. What do you understand by in UV spectroscopy
5. On what factors does the conductance of an electrolytic solution depend?
6. What is differential scanning calorimetry? Discuss the principal involved and the instrumentation used. How is the technique helpful in determining the enthalpies of transitions?
7. Discuss the principle involved in flame –photometry. Give a brief account of its applications.
8. What is flame-photometry? Describe the working of a common flame-photometer and give a brief account of the important applications of the technique.
9. Give a brief account of the vibrational- rotational spectra of diatomic molecules.
10. What are conductometric titrations? Give an account of the principle and the method of the technique.
11. In conductometric titrations, more concentrated solution is added from the burette, why? Explain the conductometric titration of a strong acid against a strong base.
12. Explain the following conductometric titrations:
i) titration of a weak acid against a strong base
ii) Titration of a strong acid against a weak base
iii) Titration of AgNO3 against KCl.
13. Explain the basic principle involved in the thermogravimetric analysis. What is its use in the structural determination of compounds?
14. What is meant by thermal analysis? Explain the functioning of DTA using block diagram.
ANALYTICAL METHODS
1. What is Thermogravimetric analysis? Describe briefly.
2. What do you understand by a thermogram and a differential thermogram?
3. What do you understand by hypsochromic shift and bathochromic shift?
4. What do you understand by in UV spectroscopy
5. On what factors does the conductance of an electrolytic solution depend?
6. What is differential scanning calorimetry? Discuss the principal involved and the instrumentation used. How is the technique helpful in determining the enthalpies of transitions?
7. Discuss the principle involved in flame –photometry. Give a brief account of its applications.
8. What is flame-photometry? Describe the working of a common flame-photometer and give a brief account of the important applications of the technique.
9. Give a brief account of the vibrational- rotational spectra of diatomic molecules.
10. What are conductometric titrations? Give an account of the principle and the method of the technique.
11. In conductometric titrations, more concentrated solution is added from the burette, why? Explain the conductometric titration of a strong acid against a strong base.
12. Explain the following conductometric titrations:
i) titration of a weak acid against a strong base
ii) Titration of a strong acid against a weak base
iii) Titration of AgNO3 against KCl.
13. Explain the basic principle involved in the thermogravimetric analysis. What is its use in the structural determination of compounds?
14. What is meant by thermal analysis? Explain the functioning of DTA using block diagram.
Tutorial-7
TUTE SHEET-7
LUBRICATION & LUBRICANTS
1. Define the following terms:
(a) Lubricant (b) Viscosity index (c) Aqua- Dag (d) Oil_dag (e) Cloud point (f) Pour Point (g) Flash Point (h) Fire point (i) Drop point (j) Aniline point (h) Oiliness.
2. Write short notes on :
(a)Carbon residue test (b) Petrol based lubricants (c) solid lubricants (d) Manufacture of grease (e) silicon lubricants (f) dibasic and esters
3. What are the various factors that dictate the choice of the lubricants
4. Explain the different theories of lubrication.
5. How are lubricating oils classified? Provide illustrations
6. Explain the role of (a) Additives (b) Anti-oxidants (c) corrosion inhibitors (d) Pour point depressant (e) Viscosity index (f) Flash point in the study of lubricants
7. Indicate the relation between viscosity index and molecular structure. Compare vis. Index of synthetic lubricants with that of mineral lubricants.
8. How do the activities functions in lubricants?
9. Explain boundary lubrications?
10. What are the functions of lubricants?
11. Write a note on solid lubricants.
12. How do extreme pressure additive work?
13. Why does graphite act as a lubricant?
14. What is axle grease and how is it prepared ?
15. Give some example of animal and vegetable oils. What are their inherited drawbacks in using as lubricants.
16. What are blended oils and why are they blended?
17. What are silicones ? Write their general formula.
18. What are antioxidants? Give some examples
19. What is hydrodynamic lubrication? Discuss its mechanism and explain why hydrocarbon oils are suitable for this type of lubrication.
20. Why hydrodynamic lubrication not possible under boundary conditions? Give a brief account of boundary lubrication and discuss its important features.
21. Write short notes on :
(i) cutting oil, (ii) cooling liquids, (iii) Blended oils, (iv) Saponification number, (v) Acid number, (vi) precipitation number, (vii) Ash content.
TUTE SHEET-7
LUBRICATION & LUBRICANTS
1. Define the following terms:
(a) Lubricant (b) Viscosity index (c) Aqua- Dag (d) Oil_dag (e) Cloud point (f) Pour Point (g) Flash Point (h) Fire point (i) Drop point (j) Aniline point (h) Oiliness.
2. Write short notes on :
(a)Carbon residue test (b) Petrol based lubricants (c) solid lubricants (d) Manufacture of grease (e) silicon lubricants (f) dibasic and esters
3. What are the various factors that dictate the choice of the lubricants
4. Explain the different theories of lubrication.
5. How are lubricating oils classified? Provide illustrations
6. Explain the role of (a) Additives (b) Anti-oxidants (c) corrosion inhibitors (d) Pour point depressant (e) Viscosity index (f) Flash point in the study of lubricants
7. Indicate the relation between viscosity index and molecular structure. Compare vis. Index of synthetic lubricants with that of mineral lubricants.
8. How do the activities functions in lubricants?
9. Explain boundary lubrications?
10. What are the functions of lubricants?
11. Write a note on solid lubricants.
12. How do extreme pressure additive work?
13. Why does graphite act as a lubricant?
14. What is axle grease and how is it prepared ?
15. Give some example of animal and vegetable oils. What are their inherited drawbacks in using as lubricants.
16. What are blended oils and why are they blended?
17. What are silicones ? Write their general formula.
18. What are antioxidants? Give some examples
19. What is hydrodynamic lubrication? Discuss its mechanism and explain why hydrocarbon oils are suitable for this type of lubrication.
20. Why hydrodynamic lubrication not possible under boundary conditions? Give a brief account of boundary lubrication and discuss its important features.
21. Write short notes on :
(i) cutting oil, (ii) cooling liquids, (iii) Blended oils, (iv) Saponification number, (v) Acid number, (vi) precipitation number, (vii) Ash content.
TUTE SHEET-7
LUBRICATION & LUBRICANTS
1. Define the following terms:
(a) Lubricant (b) Viscosity index (c) Aqua- Dag (d) Oil_dag (e) Cloud point (f) Pour Point (g) Flash Point (h) Fire point (i) Drop point (j) Aniline point (h) Oiliness.
2. Write short notes on :
(a)Carbon residue test (b) Petrol based lubricants (c) solid lubricants (d) Manufacture of grease (e) silicon lubricants (f) dibasic and esters
3. What are the various factors that dictate the choice of the lubricants
4. Explain the different theories of lubrication.
5. How are lubricating oils classified? Provide illustrations
6. Explain the role of (a) Additives (b) Anti-oxidants (c) corrosion inhibitors (d) Pour point depressant (e) Viscosity index (f) Flash point in the study of lubricants
7. Indicate the relation between viscosity index and molecular structure. Compare vis. Index of synthetic lubricants with that of mineral lubricants.
8. How do the activities functions in lubricants?
9. Explain boundary lubrications?
10. What are the functions of lubricants?
11. Write a note on solid lubricants.
12. How do extreme pressure additive work?
13. Why does graphite act as a lubricant?
14. What is axle grease and how is it prepared ?
15. Give some example of animal and vegetable oils. What are their inherited drawbacks in using as lubricants.
16. What are blended oils and why are they blended?
17. What are silicones ? Write their general formula.
18. What are antioxidants? Give some examples
19. What is hydrodynamic lubrication? Discuss its mechanism and explain why hydrocarbon oils are suitable for this type of lubrication.
20. Why hydrodynamic lubrication not possible under boundary conditions? Give a brief account of boundary lubrication and discuss its important features.
21. Write short notes on :
(i) cutting oil, (ii) cooling liquids, (iii) Blended oils, (iv) Saponification number, (v) Acid number, (vi) precipitation number, (vii) Ash content.
TUTE SHEET-7
LUBRICATION & LUBRICANTS
1. Define the following terms:
(a) Lubricant (b) Viscosity index (c) Aqua- Dag (d) Oil_dag (e) Cloud point (f) Pour Point (g) Flash Point (h) Fire point (i) Drop point (j) Aniline point (h) Oiliness.
2. Write short notes on :
(a)Carbon residue test (b) Petrol based lubricants (c) solid lubricants (d) Manufacture of grease (e) silicon lubricants (f) dibasic and esters
3. What are the various factors that dictate the choice of the lubricants
4. Explain the different theories of lubrication.
5. How are lubricating oils classified? Provide illustrations
6. Explain the role of (a) Additives (b) Anti-oxidants (c) corrosion inhibitors (d) Pour point depressant (e) Viscosity index (f) Flash point in the study of lubricants
7. Indicate the relation between viscosity index and molecular structure. Compare vis. Index of synthetic lubricants with that of mineral lubricants.
8. How do the activities functions in lubricants?
9. Explain boundary lubrications?
10. What are the functions of lubricants?
11. Write a note on solid lubricants.
12. How do extreme pressure additive work?
13. Why does graphite act as a lubricant?
14. What is axle grease and how is it prepared ?
15. Give some example of animal and vegetable oils. What are their inherited drawbacks in using as lubricants.
16. What are blended oils and why are they blended?
17. What are silicones ? Write their general formula.
18. What are antioxidants? Give some examples
19. What is hydrodynamic lubrication? Discuss its mechanism and explain why hydrocarbon oils are suitable for this type of lubrication.
20. Why hydrodynamic lubrication not possible under boundary conditions? Give a brief account of boundary lubrication and discuss its important features.
21. Write short notes on :
(i) cutting oil, (ii) cooling liquids, (iii) Blended oils, (iv) Saponification number, (v) Acid number, (vi) precipitation number, (vii) Ash content.
TUTE SHEET-7
LUBRICATION & LUBRICANTS
1. Define the following terms:
(a) Lubricant (b) Viscosity index (c) Aqua- Dag (d) Oil_dag (e) Cloud point (f) Pour Point (g) Flash Point (h) Fire point (i) Drop point (j) Aniline point (h) Oiliness.
2. Write short notes on :
(a)Carbon residue test (b) Petrol based lubricants (c) solid lubricants (d) Manufacture of grease (e) silicon lubricants (f) dibasic and esters
3. What are the various factors that dictate the choice of the lubricants
4. Explain the different theories of lubrication.
5. How are lubricating oils classified? Provide illustrations
6. Explain the role of (a) Additives (b) Anti-oxidants (c) corrosion inhibitors (d) Pour point depressant (e) Viscosity index (f) Flash point in the study of lubricants
7. Indicate the relation between viscosity index and molecular structure. Compare vis. Index of synthetic lubricants with that of mineral lubricants.
8. How do the activities functions in lubricants?
9. Explain boundary lubrications?
10. What are the functions of lubricants?
11. Write a note on solid lubricants.
12. How do extreme pressure additive work?
13. Why does graphite act as a lubricant?
14. What is axle grease and how is it prepared ?
15. Give some example of animal and vegetable oils. What are their inherited drawbacks in using as lubricants.
16. What are blended oils and why are they blended?
17. What are silicones ? Write their general formula.
18. What are antioxidants? Give some examples
19. What is hydrodynamic lubrication? Discuss its mechanism and explain why hydrocarbon oils are suitable for this type of lubrication.
20. Why hydrodynamic lubrication not possible under boundary conditions? Give a brief account of boundary lubrication and discuss its important features.
21. Write short notes on :
(i) cutting oil, (ii) cooling liquids, (iii) Blended oils, (iv) Saponification number, (v) Acid number, (vi) precipitation number, (vii) Ash content.
LUBRICATION & LUBRICANTS
1. Define the following terms:
(a) Lubricant (b) Viscosity index (c) Aqua- Dag (d) Oil_dag (e) Cloud point (f) Pour Point (g) Flash Point (h) Fire point (i) Drop point (j) Aniline point (h) Oiliness.
2. Write short notes on :
(a)Carbon residue test (b) Petrol based lubricants (c) solid lubricants (d) Manufacture of grease (e) silicon lubricants (f) dibasic and esters
3. What are the various factors that dictate the choice of the lubricants
4. Explain the different theories of lubrication.
5. How are lubricating oils classified? Provide illustrations
6. Explain the role of (a) Additives (b) Anti-oxidants (c) corrosion inhibitors (d) Pour point depressant (e) Viscosity index (f) Flash point in the study of lubricants
7. Indicate the relation between viscosity index and molecular structure. Compare vis. Index of synthetic lubricants with that of mineral lubricants.
8. How do the activities functions in lubricants?
9. Explain boundary lubrications?
10. What are the functions of lubricants?
11. Write a note on solid lubricants.
12. How do extreme pressure additive work?
13. Why does graphite act as a lubricant?
14. What is axle grease and how is it prepared ?
15. Give some example of animal and vegetable oils. What are their inherited drawbacks in using as lubricants.
16. What are blended oils and why are they blended?
17. What are silicones ? Write their general formula.
18. What are antioxidants? Give some examples
19. What is hydrodynamic lubrication? Discuss its mechanism and explain why hydrocarbon oils are suitable for this type of lubrication.
20. Why hydrodynamic lubrication not possible under boundary conditions? Give a brief account of boundary lubrication and discuss its important features.
21. Write short notes on :
(i) cutting oil, (ii) cooling liquids, (iii) Blended oils, (iv) Saponification number, (v) Acid number, (vi) precipitation number, (vii) Ash content.
TUTE SHEET-7
LUBRICATION & LUBRICANTS
1. Define the following terms:
(a) Lubricant (b) Viscosity index (c) Aqua- Dag (d) Oil_dag (e) Cloud point (f) Pour Point (g) Flash Point (h) Fire point (i) Drop point (j) Aniline point (h) Oiliness.
2. Write short notes on :
(a)Carbon residue test (b) Petrol based lubricants (c) solid lubricants (d) Manufacture of grease (e) silicon lubricants (f) dibasic and esters
3. What are the various factors that dictate the choice of the lubricants
4. Explain the different theories of lubrication.
5. How are lubricating oils classified? Provide illustrations
6. Explain the role of (a) Additives (b) Anti-oxidants (c) corrosion inhibitors (d) Pour point depressant (e) Viscosity index (f) Flash point in the study of lubricants
7. Indicate the relation between viscosity index and molecular structure. Compare vis. Index of synthetic lubricants with that of mineral lubricants.
8. How do the activities functions in lubricants?
9. Explain boundary lubrications?
10. What are the functions of lubricants?
11. Write a note on solid lubricants.
12. How do extreme pressure additive work?
13. Why does graphite act as a lubricant?
14. What is axle grease and how is it prepared ?
15. Give some example of animal and vegetable oils. What are their inherited drawbacks in using as lubricants.
16. What are blended oils and why are they blended?
17. What are silicones ? Write their general formula.
18. What are antioxidants? Give some examples
19. What is hydrodynamic lubrication? Discuss its mechanism and explain why hydrocarbon oils are suitable for this type of lubrication.
20. Why hydrodynamic lubrication not possible under boundary conditions? Give a brief account of boundary lubrication and discuss its important features.
21. Write short notes on :
(i) cutting oil, (ii) cooling liquids, (iii) Blended oils, (iv) Saponification number, (v) Acid number, (vi) precipitation number, (vii) Ash content.
TUTE SHEET-7
LUBRICATION & LUBRICANTS
1. Define the following terms:
(a) Lubricant (b) Viscosity index (c) Aqua- Dag (d) Oil_dag (e) Cloud point (f) Pour Point (g) Flash Point (h) Fire point (i) Drop point (j) Aniline point (h) Oiliness.
2. Write short notes on :
(a)Carbon residue test (b) Petrol based lubricants (c) solid lubricants (d) Manufacture of grease (e) silicon lubricants (f) dibasic and esters
3. What are the various factors that dictate the choice of the lubricants
4. Explain the different theories of lubrication.
5. How are lubricating oils classified? Provide illustrations
6. Explain the role of (a) Additives (b) Anti-oxidants (c) corrosion inhibitors (d) Pour point depressant (e) Viscosity index (f) Flash point in the study of lubricants
7. Indicate the relation between viscosity index and molecular structure. Compare vis. Index of synthetic lubricants with that of mineral lubricants.
8. How do the activities functions in lubricants?
9. Explain boundary lubrications?
10. What are the functions of lubricants?
11. Write a note on solid lubricants.
12. How do extreme pressure additive work?
13. Why does graphite act as a lubricant?
14. What is axle grease and how is it prepared ?
15. Give some example of animal and vegetable oils. What are their inherited drawbacks in using as lubricants.
16. What are blended oils and why are they blended?
17. What are silicones ? Write their general formula.
18. What are antioxidants? Give some examples
19. What is hydrodynamic lubrication? Discuss its mechanism and explain why hydrocarbon oils are suitable for this type of lubrication.
20. Why hydrodynamic lubrication not possible under boundary conditions? Give a brief account of boundary lubrication and discuss its important features.
21. Write short notes on :
(i) cutting oil, (ii) cooling liquids, (iii) Blended oils, (iv) Saponification number, (v) Acid number, (vi) precipitation number, (vii) Ash content.
TUTE SHEET-7
LUBRICATION & LUBRICANTS
1. Define the following terms:
(a) Lubricant (b) Viscosity index (c) Aqua- Dag (d) Oil_dag (e) Cloud point (f) Pour Point (g) Flash Point (h) Fire point (i) Drop point (j) Aniline point (h) Oiliness.
2. Write short notes on :
(a)Carbon residue test (b) Petrol based lubricants (c) solid lubricants (d) Manufacture of grease (e) silicon lubricants (f) dibasic and esters
3. What are the various factors that dictate the choice of the lubricants
4. Explain the different theories of lubrication.
5. How are lubricating oils classified? Provide illustrations
6. Explain the role of (a) Additives (b) Anti-oxidants (c) corrosion inhibitors (d) Pour point depressant (e) Viscosity index (f) Flash point in the study of lubricants
7. Indicate the relation between viscosity index and molecular structure. Compare vis. Index of synthetic lubricants with that of mineral lubricants.
8. How do the activities functions in lubricants?
9. Explain boundary lubrications?
10. What are the functions of lubricants?
11. Write a note on solid lubricants.
12. How do extreme pressure additive work?
13. Why does graphite act as a lubricant?
14. What is axle grease and how is it prepared ?
15. Give some example of animal and vegetable oils. What are their inherited drawbacks in using as lubricants.
16. What are blended oils and why are they blended?
17. What are silicones ? Write their general formula.
18. What are antioxidants? Give some examples
19. What is hydrodynamic lubrication? Discuss its mechanism and explain why hydrocarbon oils are suitable for this type of lubrication.
20. Why hydrodynamic lubrication not possible under boundary conditions? Give a brief account of boundary lubrication and discuss its important features.
21. Write short notes on :
(i) cutting oil, (ii) cooling liquids, (iii) Blended oils, (iv) Saponification number, (v) Acid number, (vi) precipitation number, (vii) Ash content.
TUTE SHEET-7
LUBRICATION & LUBRICANTS
1. Define the following terms:
(a) Lubricant (b) Viscosity index (c) Aqua- Dag (d) Oil_dag (e) Cloud point (f) Pour Point (g) Flash Point (h) Fire point (i) Drop point (j) Aniline point (h) Oiliness.
2. Write short notes on :
(a)Carbon residue test (b) Petrol based lubricants (c) solid lubricants (d) Manufacture of grease (e) silicon lubricants (f) dibasic and esters
3. What are the various factors that dictate the choice of the lubricants
4. Explain the different theories of lubrication.
5. How are lubricating oils classified? Provide illustrations
6. Explain the role of (a) Additives (b) Anti-oxidants (c) corrosion inhibitors (d) Pour point depressant (e) Viscosity index (f) Flash point in the study of lubricants
7. Indicate the relation between viscosity index and molecular structure. Compare vis. Index of synthetic lubricants with that of mineral lubricants.
8. How do the activities functions in lubricants?
9. Explain boundary lubrications?
10. What are the functions of lubricants?
11. Write a note on solid lubricants.
12. How do extreme pressure additive work?
13. Why does graphite act as a lubricant?
14. What is axle grease and how is it prepared ?
15. Give some example of animal and vegetable oils. What are their inherited drawbacks in using as lubricants.
16. What are blended oils and why are they blended?
17. What are silicones ? Write their general formula.
18. What are antioxidants? Give some examples
19. What is hydrodynamic lubrication? Discuss its mechanism and explain why hydrocarbon oils are suitable for this type of lubrication.
20. Why hydrodynamic lubrication not possible under boundary conditions? Give a brief account of boundary lubrication and discuss its important features.
21. Write short notes on :
(i) cutting oil, (ii) cooling liquids, (iii) Blended oils, (iv) Saponification number, (v) Acid number, (vi) precipitation number, (vii) Ash content.
Tutorial-6
TUTE-SHEET-6
POLYMERS & POLYMERISATION
1. Explain the following terms with suitable examples
(a) Monomer (b) Polymer (c) Degree of polymerization (d) Functionality (e) Homopolymers and copolymers (f) Inorganic polymers (g) Composites (h) Silicones ( i ) Elastomers
( j ) Block copolymer & Graft copolymer
( k ) Additives in polymers (l) Glass transition temperature.
2. How do you classify the polymer on the basis of :
a) Occurance in nature.
b) Monomer unit.
c) Polymeric structure.
d) Monomeric unit in backbone.
e) Tacticity.
f) Synthesis (chemical combination).
g) Arrangement of monomers in the formation of copolymers.
3. What do you understand by polymerization? Explain the mechanism of following with suitable examples:
i) Addition Polymerization (Chain growth)
a) Free radical Polymerization.
b) Cationic and Anionic polymerization
c) Coordination (Ziegler Natta / Stereo selective) polymerization.
ii) Condensation polymerizations / step growth polymerization.
4. Explain the effect of structure on polymer properties.
5. Differentiate following
a) Thermoplastics and Thermosetting polymers / resins
b) Addition and condensation polymerization
c) Synthetic and Natural rubber
d) Low density polythene (LDPE) & High density polythene (HDPE)
POLYMERS & POLYMERISATION
1. Explain the following terms with suitable examples
(a) Monomer (b) Polymer (c) Degree of polymerization (d) Functionality (e) Homopolymers and copolymers (f) Inorganic polymers (g) Composites (h) Silicones ( i ) Elastomers
( j ) Block copolymer & Graft copolymer
( k ) Additives in polymers (l) Glass transition temperature.
2. How do you classify the polymer on the basis of :
a) Occurance in nature.
b) Monomer unit.
c) Polymeric structure.
d) Monomeric unit in backbone.
e) Tacticity.
f) Synthesis (chemical combination).
g) Arrangement of monomers in the formation of copolymers.
3. What do you understand by polymerization? Explain the mechanism of following with suitable examples:
i) Addition Polymerization (Chain growth)
a) Free radical Polymerization.
b) Cationic and Anionic polymerization
c) Coordination (Ziegler Natta / Stereo selective) polymerization.
ii) Condensation polymerizations / step growth polymerization.
4. Explain the effect of structure on polymer properties.
5. Differentiate following
a) Thermoplastics and Thermosetting polymers / resins
b) Addition and condensation polymerization
c) Synthetic and Natural rubber
d) Low density polythene (LDPE) & High density polythene (HDPE)
Tutorial-5
TUTE –SHEET-5
CORROSION
1. Define corrosion . What are different types of corrosion? Explain the electrochemical theory of wet corrosion, giving its mechanism.
2. (a) Explain rusting of Iron with the help of electrochemical theory of corrosion.
(b) Differentiate between chemical corrosion and electrochemical corrosion.
(c) What will happen when stainless is immersed in aerated and de aerated sodium chloride solution?
3. (a) Write chemical reaction taking place during stress corrosion of brass.
(b) Illustrate the reactions involved in differential aeration corrosion with difference to the iron materials.
4. Explain the mechanism of following types of corrosions.
a) Chemical corrosion
b) Stress corrosion
c) Water-line corrosion
d) Pitting corrosion
e) Bimetallic or galvanic corrosion
5. (a) Mention different methods used for prevention of corrosion of metals and discuss any one of them.
(b) Write short notes on cathodic protection.
6. (a) Why impure metal are more susceptible to corrosion than pure metals?
(b) What are the factors, which affect corrosion?
7. What are metallic coatings? Explain the functioning of two types of metallic coatings. Explain the methods employed for coating metals.
8. Write short notes on the following:
(i) Electroplating, (ii) Metal Cladding.
9. What are electrochemical and galvanic series? Distinguish between the two and point out their role in corrosion.
10. What is sacrificial protection from corrosion? Give examples and explain any one in detail.
11. What are corrosion inhibitors ? Give some examples of organic and inorganic inhibitors. Enlist two applications where voltage inhibitors are used.
CORROSION
1. Define corrosion . What are different types of corrosion? Explain the electrochemical theory of wet corrosion, giving its mechanism.
2. (a) Explain rusting of Iron with the help of electrochemical theory of corrosion.
(b) Differentiate between chemical corrosion and electrochemical corrosion.
(c) What will happen when stainless is immersed in aerated and de aerated sodium chloride solution?
3. (a) Write chemical reaction taking place during stress corrosion of brass.
(b) Illustrate the reactions involved in differential aeration corrosion with difference to the iron materials.
4. Explain the mechanism of following types of corrosions.
a) Chemical corrosion
b) Stress corrosion
c) Water-line corrosion
d) Pitting corrosion
e) Bimetallic or galvanic corrosion
5. (a) Mention different methods used for prevention of corrosion of metals and discuss any one of them.
(b) Write short notes on cathodic protection.
6. (a) Why impure metal are more susceptible to corrosion than pure metals?
(b) What are the factors, which affect corrosion?
7. What are metallic coatings? Explain the functioning of two types of metallic coatings. Explain the methods employed for coating metals.
8. Write short notes on the following:
(i) Electroplating, (ii) Metal Cladding.
9. What are electrochemical and galvanic series? Distinguish between the two and point out their role in corrosion.
10. What is sacrificial protection from corrosion? Give examples and explain any one in detail.
11. What are corrosion inhibitors ? Give some examples of organic and inorganic inhibitors. Enlist two applications where voltage inhibitors are used.
Tutorial-4
TUTE- SHEET-4
WATER TREATMENT-2
1. What are Zeolites and what for they used?
2. How are exhausted resins regenerated in an exchange process? Write the chemical reactions involved.
3. What are the advantages of using chloramines as a disinfectant?
4. What is break-point chlorination?
5. What do you understand by softening of water? Describe the lime soda process and elaborate the functions of lime and soda in the process.
6. Describe hot lime- soda process used for the softening of water. In what respect is this process superior to the cold lime-soda process? What are the limitations of the process?
7. Describe the zeolite process used for softening of water. What are the advantages and limitations of the process?
8. Describe the demineralization process for softening of water. What are its advantages and limitations?
9. What are the essential qualities of drinking water? Describe the various process used for domestic water treatment.
10. Explain the following term.
a) Chlorination, b) Super chlorination, c) De chlorination, d) Break-point chlorination
11. Calculate the amount of lime and soda required for softening of 15000 liter of water, which analysed as follow : Temporary hardness =20 ppm, Permanent hardness = 15 ppm, permanent Mg hardness = 10 ppm.
WATER TREATMENT-2
1. What are Zeolites and what for they used?
2. How are exhausted resins regenerated in an exchange process? Write the chemical reactions involved.
3. What are the advantages of using chloramines as a disinfectant?
4. What is break-point chlorination?
5. What do you understand by softening of water? Describe the lime soda process and elaborate the functions of lime and soda in the process.
6. Describe hot lime- soda process used for the softening of water. In what respect is this process superior to the cold lime-soda process? What are the limitations of the process?
7. Describe the zeolite process used for softening of water. What are the advantages and limitations of the process?
8. Describe the demineralization process for softening of water. What are its advantages and limitations?
9. What are the essential qualities of drinking water? Describe the various process used for domestic water treatment.
10. Explain the following term.
a) Chlorination, b) Super chlorination, c) De chlorination, d) Break-point chlorination
11. Calculate the amount of lime and soda required for softening of 15000 liter of water, which analysed as follow : Temporary hardness =20 ppm, Permanent hardness = 15 ppm, permanent Mg hardness = 10 ppm.
Tutorial-3
TUTE SHEET- 3
WATER TREATMENT-1
1.
1. Rainwater is the purest form of natural resource of water. Why?
2. What are the different sources of water also elaborate the uses of water?
3. Explain the different types of impurities present in water.
4. How would you explain the term Hardness of water?
5. Name the salts, which cause permanent and temporary hardness to the water.
6. Why does hard water consumes lot of soap?
7. What are the different degrees of hardness and what is the relation between them?
8. Why do we express hardness of water in terms of CaCO3 equivalent?
9. 100ml of water sample has hardness equivalent to 12.5ml of 0.08N MgSO4. What is
the hardness in ppm ?
10. A water sample contains 204mg of CaSO4/L, Calculate the hardness in terms of
CaCO3 equivalent.
11. Calculate the total, temporary, and, permanent hardness of water sample containing
following per liter Ca(HCO3)2= 162mg, Mg(HCO3)2= 73mg , MgCl2= 95mg,CaSO4= 136mg.
12. What are the units of hardness?
13. Define alkalinity. How is it determined?
14. What do you understand by scale and sludge? How are they formed? What are their disadvantages and how are they prevented?
15. Why Calgon conditioning is better than Phosphate Conditioning?
16. Write a short note on caustic embrittlement and boiler corrosion.
17. Describe the EDTA method for the estimation of hardness of water.
18. 200 ml. of water sample required 25 ml. Of N/50 H2SO4 during titration by using phenolphthalein indicator and 26 ml. of acid by using methyl orange indicator. Calculate the alkalinity of each type in terms of CaCO3 equivalent.
19. 100 ml. of a water sample required 4 ml. of N/50 H2SO4 for neutralization to phenolphthalein end point. Another 16 ml. of same acid was needed for further titration to methyl orange end point. Determine the type and amount of alkalinity.
20. 200 ml. of hard water sample require 30 ml. of 0.02 M of EDTA with buffer and EBT indicator. Another 200 ml. of the sample is boiled for about half an hour and filtering the ppt., the volume of filterate is made 200 ml. by the addition of distilled water. 20 ml. of this boiled water sample required 5 ml. of 0.01M EDTA following the same procedure. Calculate the temporary and permanent hardness of the sample.
21. A standard hard water contains 15 gm. Of CaCO3 per litre. 20 ml. of this required 25 ml. of EDTA soln., 100 ml. of sample water required 18 ml. of EDTA soln. The sample after boiling required 12 ml. EDTA soln. Calculate the temporary hardness of the given sample of water, in terms of ppm.
22. Calculate the hardness of a water sample, whose 10 ml. required 10 ml. of EDTA. 20 ml. of CaCl2 solution, whose strength is equivalent 1.5 gm. Of CaCO3 per litre, required 30 ml. of EDTA solution.
WATER TREATMENT-1
1.
1. Rainwater is the purest form of natural resource of water. Why?
2. What are the different sources of water also elaborate the uses of water?
3. Explain the different types of impurities present in water.
4. How would you explain the term Hardness of water?
5. Name the salts, which cause permanent and temporary hardness to the water.
6. Why does hard water consumes lot of soap?
7. What are the different degrees of hardness and what is the relation between them?
8. Why do we express hardness of water in terms of CaCO3 equivalent?
9. 100ml of water sample has hardness equivalent to 12.5ml of 0.08N MgSO4. What is
the hardness in ppm ?
10. A water sample contains 204mg of CaSO4/L, Calculate the hardness in terms of
CaCO3 equivalent.
11. Calculate the total, temporary, and, permanent hardness of water sample containing
following per liter Ca(HCO3)2= 162mg, Mg(HCO3)2= 73mg , MgCl2= 95mg,CaSO4= 136mg.
12. What are the units of hardness?
13. Define alkalinity. How is it determined?
14. What do you understand by scale and sludge? How are they formed? What are their disadvantages and how are they prevented?
15. Why Calgon conditioning is better than Phosphate Conditioning?
16. Write a short note on caustic embrittlement and boiler corrosion.
17. Describe the EDTA method for the estimation of hardness of water.
18. 200 ml. of water sample required 25 ml. Of N/50 H2SO4 during titration by using phenolphthalein indicator and 26 ml. of acid by using methyl orange indicator. Calculate the alkalinity of each type in terms of CaCO3 equivalent.
19. 100 ml. of a water sample required 4 ml. of N/50 H2SO4 for neutralization to phenolphthalein end point. Another 16 ml. of same acid was needed for further titration to methyl orange end point. Determine the type and amount of alkalinity.
20. 200 ml. of hard water sample require 30 ml. of 0.02 M of EDTA with buffer and EBT indicator. Another 200 ml. of the sample is boiled for about half an hour and filtering the ppt., the volume of filterate is made 200 ml. by the addition of distilled water. 20 ml. of this boiled water sample required 5 ml. of 0.01M EDTA following the same procedure. Calculate the temporary and permanent hardness of the sample.
21. A standard hard water contains 15 gm. Of CaCO3 per litre. 20 ml. of this required 25 ml. of EDTA soln., 100 ml. of sample water required 18 ml. of EDTA soln. The sample after boiling required 12 ml. EDTA soln. Calculate the temporary hardness of the given sample of water, in terms of ppm.
22. Calculate the hardness of a water sample, whose 10 ml. required 10 ml. of EDTA. 20 ml. of CaCl2 solution, whose strength is equivalent 1.5 gm. Of CaCO3 per litre, required 30 ml. of EDTA solution.
Tutorial-2
TUTE SHEET- 2
PHASE RULE
1. State the Phase-Rule and describe following terminologies with as many as appropriate examples:
(a) Phase (b) Component (c) Degree of Freedom
(d) Metastable equilibrium (e) Eutectic Point (f) Congruent Melting Point
(g) Incongruent Melting Point (h) Cooling curves (i) Triple point
(j) Phase Diagrams. (k) Eutectic system and mixtures.
2. Derive Gibb’s Phase Rule.
3. Write a note on ‘reduced phase rule’.
4. With the help of neat and labeled Phase-diagram explain the following systems (considering Curves, Areas point and F)
(a) Water system
(b) Ag-Pb system
(c) Na – K system
(d) Zn – Mg system
5. Calculate the number of components and degree of freedom for the decomposition of NH4Cl.
NH4Cl(s) NH3(g) + HCl(g) ; PNH3 = PHCl
6. Discuss the merits and limitations of phase rule.
7. Calculate the number of components present in the following:
(a) CaCO3(s) CaO(s) + CO2(g)
(b) Ag(s) Ag-Pb solution (l) + Pb-Ag vapour (g)
(c) NH4Cl (s) xNH3 (q) + y HCl (g)
(d) Fe(s) + H2O (g) FeO(s) + H2 (g)
PHASE RULE
1. State the Phase-Rule and describe following terminologies with as many as appropriate examples:
(a) Phase (b) Component (c) Degree of Freedom
(d) Metastable equilibrium (e) Eutectic Point (f) Congruent Melting Point
(g) Incongruent Melting Point (h) Cooling curves (i) Triple point
(j) Phase Diagrams. (k) Eutectic system and mixtures.
2. Derive Gibb’s Phase Rule.
3. Write a note on ‘reduced phase rule’.
4. With the help of neat and labeled Phase-diagram explain the following systems (considering Curves, Areas point and F)
(a) Water system
(b) Ag-Pb system
(c) Na – K system
(d) Zn – Mg system
5. Calculate the number of components and degree of freedom for the decomposition of NH4Cl.
NH4Cl(s) NH3(g) + HCl(g) ; PNH3 = PHCl
6. Discuss the merits and limitations of phase rule.
7. Calculate the number of components present in the following:
(a) CaCO3(s) CaO(s) + CO2(g)
(b) Ag(s) Ag-Pb solution (l) + Pb-Ag vapour (g)
(c) NH4Cl (s) xNH3 (q) + y HCl (g)
(d) Fe(s) + H2O (g) FeO(s) + H2 (g)
Tutorial-1
TUTE SHEET- 1
THERMODYNAMICS
1. Explain following with suitable examples.
Homogeneous and Heterogeneous system, Intensive and Extensive properties. Reversible and Irreversible process. Work, internal energy and heat, 1st law of thermodynamics. Also mention the units of DH, DS, q, w, E, DG, in SI and CGS systems.
2. Define enthalpy. Why is the enthalpy change, regarded as a measure of heat change involved in a process accruing at constant pressure?
3. Prove DH = qp; DH = DE +D ngRT; -(DG) = Wmax; and –(DA) = Wmax - PDV
4. Define heat capacity.
5. Show that Cp – Cv = R
6. What do you understand by spontaneous process? Give some example.
7. Define entropy and discuss its physical significance.
8. Derive the expression for entropy change for an Ideal gas.
9. The enthalpy change for the transition of liquid water to steam DH vap is 40.8KJmol-1 at 1000C. Calculate the entropy change (DSvap) for the process. (Ans 109.38J/K.mol)
10. Two moles of an ideal gas expand isothermally and reversibly from a volume of 10 dm3 to 20dm3 at 300 K calculate the entropy change involved. (Ans. 11.53JK-1).
11. One mole of an ideal gas (monatomic) expands reversibly from a volume of 5dm3 to 10 dm3 and temperature 300K to a volume of 25dm3 and temperature 230K. Assuming that Cv = 3/2 R. Calculate DS for the process. (Ans. 4.305 JK-1 mol-1)
12. Calculate the change in entropy accompanying the heating of one mole of helium gas, assumed ideal, from a temperature 298K to a temperature at 1000K at constant pressure. Assume the Cv=3/2R (Ans. 25.17 JK-1mol-1)
13. One mole of an ideal gas heated from 100K to 300K. Calculate DS, if (i) the volume is kept constant (ii) the pressure is kept constant. Assume that Cv = 1.5R (Ans. 13.17 JK-1 ; 22.8JK-1 mol–1).
14. What do you understand by a spontaneous process and spontaneity of a process? Discuss the spontaneity of a process in terms of Gibbs free energy change.
15. What was the need to introduce the 2nd Law thermodynamics? State the law by five different ways & also give justification for 1st law of thermodynamics.
16. Show that decrease in change in free energy in a process is a measure of the maximum work (reversible work) done by the system.
17. Show that decrease in change in Helmholtz free energy function (work function) gives the max. work that can be obtained from a system during the change at constant temperature & pressure.
18. Derive the relation, dG = Vdp – sdT, ; ;
(DG)T = 2.303 nRT log and (DA)T = 2.303nRT log v1 / v2.
19. Derive Gibbs – Helmholtz equation in terms of free energy & in terms of work function also discuss its significance.
20. Derive Clapeyron – Clausius application in its integrated form with its applications. Under what conditions it is integrated.
21. The free energy change (DG) accompanying a given process is –85.77 kJ at 250C and –83.68 KJ at 350C. Calculate the change in enthalpy (DH) for the process at 300C. (Ans. DH = - 148.05 kJ).
22. Vapour pressure of water at 950C and 1000C are 634 and 760 mm, respectively. Calculate the molar heat of vaporization, DHv, of water between 950 and 1000C. (Ans. DH = 41363J/mol)
23. The vapour pressure of water at 1000C is 760mm. What will be the vapour pressure at 950C. The heat of vapouration water in this temperature range is 41.27 kJ per mole (Ans. P2 = 634.3mm).
24. DG for a reaction at 300K is – 16 Kcal, DH for the reaction is – 10Kcal. What is entropy of the reaction? What will be DG at 330K? (Ans. DS = 0.02 Kcal or 20 cal K-1; DG = 16.6 Kcal).
25. Calculate DH, DS, DG and DE when 1 mole of water is vaporized at 1000C and 1 atm. The latent heat of vaporization of water is 540 cal/g. (Ans. DS = 26.06; DG = 0; DE = 8979.5 Cal; DH = 9,720 Cal).
26. Define chemical potential and write the symbol of that and also explain the significance of chemical potential.
27. Compute the change in chemical potential of a substance if the partial pressure of a ideal gas falls from 1.00 atom to 0.5 atm at 298K (Ans. –1,717.3 J mil-1)
28. At what temperature will water boil when the atm. Pressure is 528mm Hg? Latent heat of vap. of water is 545.5 cal/g (Ans. 363K).
29. Show that entropy change for reversible process is zero and for irreversible process it is always positive (tends to be increasing).
30. Calculate the change in volume for melting of 1 g mole of phenol. Given latent heat of fusion = 3250 cal / g mol. Melting point of phenol = 330 K; dP / dT = 287atm /K.
THERMODYNAMICS
1. Explain following with suitable examples.
Homogeneous and Heterogeneous system, Intensive and Extensive properties. Reversible and Irreversible process. Work, internal energy and heat, 1st law of thermodynamics. Also mention the units of DH, DS, q, w, E, DG, in SI and CGS systems.
2. Define enthalpy. Why is the enthalpy change, regarded as a measure of heat change involved in a process accruing at constant pressure?
3. Prove DH = qp; DH = DE +D ngRT; -(DG) = Wmax; and –(DA) = Wmax - PDV
4. Define heat capacity.
5. Show that Cp – Cv = R
6. What do you understand by spontaneous process? Give some example.
7. Define entropy and discuss its physical significance.
8. Derive the expression for entropy change for an Ideal gas.
9. The enthalpy change for the transition of liquid water to steam DH vap is 40.8KJmol-1 at 1000C. Calculate the entropy change (DSvap) for the process. (Ans 109.38J/K.mol)
10. Two moles of an ideal gas expand isothermally and reversibly from a volume of 10 dm3 to 20dm3 at 300 K calculate the entropy change involved. (Ans. 11.53JK-1).
11. One mole of an ideal gas (monatomic) expands reversibly from a volume of 5dm3 to 10 dm3 and temperature 300K to a volume of 25dm3 and temperature 230K. Assuming that Cv = 3/2 R. Calculate DS for the process. (Ans. 4.305 JK-1 mol-1)
12. Calculate the change in entropy accompanying the heating of one mole of helium gas, assumed ideal, from a temperature 298K to a temperature at 1000K at constant pressure. Assume the Cv=3/2R (Ans. 25.17 JK-1mol-1)
13. One mole of an ideal gas heated from 100K to 300K. Calculate DS, if (i) the volume is kept constant (ii) the pressure is kept constant. Assume that Cv = 1.5R (Ans. 13.17 JK-1 ; 22.8JK-1 mol–1).
14. What do you understand by a spontaneous process and spontaneity of a process? Discuss the spontaneity of a process in terms of Gibbs free energy change.
15. What was the need to introduce the 2nd Law thermodynamics? State the law by five different ways & also give justification for 1st law of thermodynamics.
16. Show that decrease in change in free energy in a process is a measure of the maximum work (reversible work) done by the system.
17. Show that decrease in change in Helmholtz free energy function (work function) gives the max. work that can be obtained from a system during the change at constant temperature & pressure.
18. Derive the relation, dG = Vdp – sdT, ; ;
(DG)T = 2.303 nRT log and (DA)T = 2.303nRT log v1 / v2.
19. Derive Gibbs – Helmholtz equation in terms of free energy & in terms of work function also discuss its significance.
20. Derive Clapeyron – Clausius application in its integrated form with its applications. Under what conditions it is integrated.
21. The free energy change (DG) accompanying a given process is –85.77 kJ at 250C and –83.68 KJ at 350C. Calculate the change in enthalpy (DH) for the process at 300C. (Ans. DH = - 148.05 kJ).
22. Vapour pressure of water at 950C and 1000C are 634 and 760 mm, respectively. Calculate the molar heat of vaporization, DHv, of water between 950 and 1000C. (Ans. DH = 41363J/mol)
23. The vapour pressure of water at 1000C is 760mm. What will be the vapour pressure at 950C. The heat of vapouration water in this temperature range is 41.27 kJ per mole (Ans. P2 = 634.3mm).
24. DG for a reaction at 300K is – 16 Kcal, DH for the reaction is – 10Kcal. What is entropy of the reaction? What will be DG at 330K? (Ans. DS = 0.02 Kcal or 20 cal K-1; DG = 16.6 Kcal).
25. Calculate DH, DS, DG and DE when 1 mole of water is vaporized at 1000C and 1 atm. The latent heat of vaporization of water is 540 cal/g. (Ans. DS = 26.06; DG = 0; DE = 8979.5 Cal; DH = 9,720 Cal).
26. Define chemical potential and write the symbol of that and also explain the significance of chemical potential.
27. Compute the change in chemical potential of a substance if the partial pressure of a ideal gas falls from 1.00 atom to 0.5 atm at 298K (Ans. –1,717.3 J mil-1)
28. At what temperature will water boil when the atm. Pressure is 528mm Hg? Latent heat of vap. of water is 545.5 cal/g (Ans. 363K).
29. Show that entropy change for reversible process is zero and for irreversible process it is always positive (tends to be increasing).
30. Calculate the change in volume for melting of 1 g mole of phenol. Given latent heat of fusion = 3250 cal / g mol. Melting point of phenol = 330 K; dP / dT = 287atm /K.
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