4

# __________ does not change during phase transformation processes like sublimation, melting & vaporisation.

Entropy

Gibbs free energy

Internal energy

All (A), (B) & (C)

B. Gibbs free energy

4

# In case of a close thermodynamic system, there is __________ across the boundaries.

No heat and mass transfer

No mass transfer but heat transfer

Mass and energy transfer

None of these

4

# Trouton's ratio of __________ liquids is calculated using Kistyakowsky equation.

Polar

Non-polar

Both (A) & (B)

Neither (A) nor (B)

4

None of these

4

# Standard temperature and pressure (S.T.P.) is

0°C and 750 mm Hg

15°C and 750 mm Hg

0°C and 1 kgf/cm2

15°C and 1 kgf/cm2

4

# Fugacity is most helpful in

Representing actual behaviour of real gases

Representing actual behaviour of ideal gases

The study of chemical equilibria involving gases at atmospheric pressure

None of these

4

# The chemical potential of any constituent of an ideal solution depends on the __________ of the solution.

Temperature

Pressure

Composition

All (A), (B) and (C)

4

# Gibbs-Duhem equation

States that n11 + n22 + ....njj = 0, for a system of definite composition at constant temperature and pressure

Applies only to binary systems

Finds no application in gas-liquid equilibria involved in distillation

None of these

4

0

1

2

3

4

# The unit of equilibrium constant of a chemical reaction is the same as that of

Molar concentration

Temperature

Internal energy

None of these

4

12 P1V1

6 P1 V1

3 P1V1

P1 V1

4

# Gibbs-Helmholtz equation is

ΔF = ΔH + T [∂(ΔF)/∂T]P

ΔF = ΔH - TΔT

d(E - TS) T, V < 0

dP/dT = ΔHvap/T.ΔVvap

4

# Change of heat content when one mole of compound is burnt in oxygen at constant pressure is called the

Calorific value

Heat of reaction

Heat of combustion

Heat of formation

4

# A gas shows deviation from ideal behaviour at

Low pressure and high temperature

Low pressure and low temperature

Low temperature and high pressure

High temperature and high pressure

4

# Compound having large heat of formation is

More stable

Less stable

Not at all stable (like nascent O2)

Either more or less stable; depends on the compound

4

# Pick out the wrong statement:

The expansion of a gas in vacuum is an irreversible process

An isometric process is a constant pressure process

Entropy change for a reversible adiabatic process is zero

Free energy change for a spontaneous process is negative

4

< 0

> 0

= 0

None of these

4

# The standard Gibbs free energy change of a reaction depends on the equilibrium

Pressure

Temperature

Composition

All (A), (B) and (C)

4

# Work done is a

Property of the system

Path function

Point function

State description of a system

4

# Lowering of condenser temperature (keeping the evaporator temperature constant) in case of vapour compression refrigeration system results in

Increased COP

Same COP

Decreased COP

Increased or decreased COP; depending upon the type of refrigerant

4

# Cp - Cv = R is valid for __________ gases.

Ideal

Very high pressure

Very low temperature

All of the above

4

# With increase in pressure (above atmospheric pressure), the Cp of a gas

Increases

Decreases

Remains unchanged

First decreases and then increases

4

# In a homogeneous solution, the activity coefficient of a component depends upon the

Pressure

Composition

Temperature

All (A), (B) and (C)

4

1st

Zeroth

3rd

None of these

4

0

1

2

3

4

# Enthalpy changes over a constant pressure path are always zero for __________ gas.

Any

A perfect

An easily liquefiable

A real

4

Zero

50%

Almost 100%

unpredictable

4

Rectangle

Rhombus

Trapezoid

Circle

4

# The equation relating E, P, V and T which is true for all substances under all conditions is given by (∂E/∂V)T = T(∂P/∂T)H - P. This equation is called the

Maxwell's equation

Thermodynamic equation of state

Equation of state

Redlich-Kwong equation of state

4

# The rate at which a substance reacts is proportional to its active mass and the rate of a chemical reaction is proportional to the product of active masses of the reacting substances. This is the

Lewis-Randall rule

Statement of Van't Hoff Equation

Le-Chatelier's principle

None of these