4

1.572

1.9398

3.389

4.238

A. 1.572

4

Stirling

Brayton

Rankine

Both (B) and (C)

4

# When a gas is expanded from high pressure region to low pressure region; temperature change occurs. This phenomenon is related to the

Gibbs-Duhem equation

Gibbs-Helmholtz equation

Third law of thermodynamics

Joule-Thomson effect

4

Conduction

Convection

Condensation

4

Free energy

Entropy

Refractive index

None of these

4

1

< 1

> 1

>> 1

4

# Mollier chart is a __________ plot.

Pressure vs. enthalpy

Pressure vs. volume

Enthalpy vs. entropy

Temperature vs. entropy

4

# If the internal energy of an ideal gas decreases by the same amount as the work done by the system, then the

Process must be isobaric

Temperature must decrease

Both (B) and (C)

4

Mass

Energy

Momentum

None of these

4

Volume

Density

Temperature

Pressure

4

# Requisites of a reversible process is that the

System and surroundings pressure be equal

Friction in the system should be absent

System and surroundings temperature be equal

None of these

4

> 2

< 1

> 1

< 3

4

# A solute distributes itself between two nonmiscible solvents in contact with each other in such a way that, at a constant temperature, the ratio of its concentrations in two layers is constant, irrespective of its total amount. This is

The distribution law

Followed from Margules equation

A corollary of Henry's law

None of these

4

# The change in __________ is equal to the reversible work for compression in steady state flow process under isothermal condition.

Internal energy

Enthalpy

Gibbs free energy

Helmholtz free energy

4

Molecular size

Temperature

Volume

Pressure

4

RT d ln P

R d ln P

R d ln f

None of these

4

# In reactions involving solids and liquids (where change in volume is negligible), the heat of reaction at constant pressure as compared to that at constant volume is

More

Less

Same

Unpredictable; depends on the particular reaction

4

# Free energy

Decreases in all spontaneous (or irreversible) processes

Change during a spontaneous process has a negative value

Remains unchanged in reversible processes carried at constant temperature and pressure

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

4

A . x22

Ax1

Ax2

Ax12

4

0

1

2

3

4

# For the gaseous phase chemical reaction, C2H4(g) + H2O(g) ↔ C2H5OH(g), the equilibrium conversion does not depend on the

Steam to ethylene ratio

Temperature

Pressure

None of these

4

# Work done in an adiabatic process between two states depends on the

Rate of heat transmission

Initial state only

End states only

None of these

4

# In a homogeneous solution, the fugacity of a component depends upon the

Pressure

Composition

Temperature

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

4

Path

Point

State

None of these

4

# Which of the following is not a reversible process?

Expansion of an ideal gas against constant pressure

Atmospheric pressure vaporisation of water at 100°C

Solution of NaCl in water at 50°C

None of these

4

-94 kcal

+94 kcal

> 94 kcal

< -94 kcal

4

# Pick out the Clausius-Clapeyron equation from the following:

dP/dT = ΔH/TΔV

ln P = - (ΔH/RT) + constant

ΔF = ΔH + T [∂(ΔF)/∂T]P

None of these

4

# Pick out the correct statement.

Entropy and enthalpy are path functions

In a closed system, the energy can be exchanged with the surrounding, while matter cannot be exchanged

All the natural processes are reversible in nature

Work is a state function

4

# The thermodynamic law, PVy = constant, is not applicable in case of

Ideal compression of air

Free expansion of an ideal gas

Adiabatic expansion of steam in a turbine

Adiabatic compression of a perfect gas

4

# Which of the following is true for Virial equation of state?

Virial co-efficients are universal constants

Virial co-efficients 'B' represents three body interactions

Virial co-efficients are function of temperature only

For some gases, Virial equations and ideal gas equations are the same