4

x

x + 1

x + 2

x + 3

C. x + 2

4

# Gibbs free energy per mole for a pure substance is equal to the

Latent heat of vaporisation

Chemical potential

Molal boiling point

Heat capacity

4

Temperature

Mass

Volume

Pressure

4

# Claude gas liquefaction process employs cooling

At constant pressure

By throttling

By expansion in an engine

None of these

4

100,000 kW

160,000 kW

200,000 kW

320,000 kW

4

# Pick out the wrong statement.

An ideal liquid or solid solution is defined as one in which each component obeys Raoult's law

If Raoult's law is applied to one component of a binary mixture; Henry's law or Raoult's law is applied to the other component also

Henry's law is rigorously correct in the limit of infinite dilution

None of these

4

# Pick out the wrong statement.

Enthalpies of all elements in their standard states are assumed to be zero

Combustion reactions are never endothermic in nature

Heat of reaction at constant volume is equal to the change in internal energy

Clausius-Clapeyron equation is not applicable to melting process

4

0

1

y = 1.44

1.66

4

Isothermal

Isometric

None of these

4

# Fugacity co-efficient of a substance is the ratio of its fugacity to

Mole fraction

Activity

Pressure

Activity co-efficient

4

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

Entropy

Gibbs free energy

Internal energy

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

4

# Compressibility factor-reduced pressure plot on reduced co-ordinates facilitates

Use of only one graph for all gases

Covering of wide range

Easier plotting

More accurate plotting

4

P + F - C = 2

C = P - F + 2

F = C - P - 2

P = F - C - 2

4

# Which of the following is not a unit of the equilibrium constant Kp? (where, Δx = number of moles of products number of moles of reactants)

(atm)Δx, when Δx is negative

(atm)Δx, when Δx is positive

Dimensionless, when Δx = 0

(atm)Δx2, when Δx > 0

4

# Entropy, which is a measure of the disorder of a system, is:

Independent of pressure

Independent of temperature

Zero at absolute zero temperature for a perfect crystalline substance

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

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

# Which of the following non-flow reversible compression processes require maximum work?

Isothermal process

Isobaric process

All require same work

4

# When dilute aqueous solutions of two salts are mixed, the process is associated with

Decrease in temperature

Increase in temperature

No change in temperature

Change in temperature which is a function of composition

4

# Pick out the wrong statement

Phase rule variables are intensive properties

Heat and work are both state function

The work done by expansion of a gas in vacuum is zero

CP and CV are state function

4

# Normal temperature and pressure (N.T.P.) corresponds to

0°C and 760 mm Hg

15°C and 760 mm Hg

20°C and 760 mm Hg

0°C and 1 kgf/cm2

4

349

651

667

1000

4

# (1/V) (∂V/∂T)P is the mathematical expression

Joule-Thomson co-efficient

Specific heat at constant pressure (Cp)

co-efficient of thermal expansion

Specific heat at constant volume (CV)

4

# First law of thermodynamics deals with the

Direction of energy transfer

Reversible processes only

Irreversible processes only

None of these

4

# An isentropic process is carried out at constant

Volume

Pressure

Temperature

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

4

# Which of the following will increase the volume of a real gas by four times?

Doubling the absolute temperature as well as pressure of the gas

Reducing pressure to one fourth at constant temperature

Reducing temperature to one fourth at constant pressure

Reducing the temperature to half and doubling the pressure

4

# The value of gas constant 'R' is

1.987 cal/gm mole °K

1.987 BTU/lb. mole °R

Both (A) and (B)

Neither (A) nor (B)

4

0.5

3.5

4.5

8.5

4

# Internal energy change of a system over one complete cycle in a cyclic process is

Zero

+ve

-ve

Dependent on the path

4

RT ln K

-RT ln K

-R ln K

T ln K

4

# If the heat of solution of an ideal gas in a liquid is negative, then its solubility at a given partial pressure varies with the temperature as

Solubility increases as temperature increases

Solubility increases as temperature decreases

Solubility is independent of temperature

Solubility increases or decreases with temperature depending on the Gibbs free energy change of solution