Always greater than one

Same at the same reduced temperature

Same at the same reduced pressure

Both (B) & (C)

D. Both (B) & (C)

√(2KT/m)

√(3KT/m)

√(6KT/m)

3KT/m

Pressure and temperature

Reduced pressure and reduced temperature

Critical pressure and critical temperature

None of these

The conversion for a gas phase reaction increases with decrease in pressure, if there is an increase in volume accompanying the reaction

With increase in temperature, the equilibrium constant increases for an exothermic reaction

The equilibrium constant of a reaction depends upon temperature only

The conversion for a gas phase reaction increases with increase in pressure, if there is a decrease in volume accompanying the reaction

Gibbs-Duhem equation

Gibbs-Helmholtz equation

Third law of thermodynamics

Joule-Thomson effect

Enthalpy

Internal energy

Either (A) or (B)

Neither (A) nor (B)

Isobaric

Adiabatic

Isenthalpic

Both (B) & (C)

_{1} is always < Δ S_{R}

_{1} is sometimes > Δ S_{R}

_{1} is always > Δ S_{R}

_{1} is always = Δ S_{R}

5 & 3

3.987 & 1.987

1.987 & 0.66

0.66 & 1.987

Addition of inert gas favours the forward reaction, when Δx is positive

Pressure has no effect on equilibrium, when Δn = 0

Addition of inert gas has no effect on the equilibrium constant at constant volume for any value of Δx (+ ve, - ve) or zero)

All 'a', 'b' & 'c'

A refrigeration cycle violates the second law of thermodynamics

Refrigeration cycle is normally represented by a temperature vs. entropy plot

In a refrigerator, work required decreases as the temperature of the refrigerator and the temperature at which heat is rejected increases

One ton of refrigeration is equivalent to the rate of heat absorption equal to 3.53 kW

Zeroth

First

Second

Third

Low pressure and high temperature

Low pressure and low temperature

High pressure and low temperature

High pressure and high temperature

-273

0

-78

5

0

< 0

< 1

> 1

Molecular size

Volume

Pressure

Temperature

Infinity

Minus infinity

Zero

None of these

Both the processes are adiabatic

Both the processes are isothermal

Process A is isothermal while B is adiabatic

Process A is adiabatic while B is isothermal

Only F decreases

Only A decreases

Both F and A decreases

Both F and A increase

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

Zeroth

First

Second

Third

_{V}

Entropy change

Gibbs free energy

None of these

Hess's

Kirchoff's

Lavoisier and Laplace

None of these

Momentum

Mass

Energy

None of these

Low pressure and high temperature

Low pressure and low temperature

Low temperature and high pressure

High temperature and high pressure

Use of only one graph for all gases

Covering of wide range

Easier plotting

More accurate plotting

^{Δx}, when Δx is negative

^{Δx}, when Δx is positive

Dimensionless, when Δx = 0

^{Δx2}, when Δx > 0

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

Solution

Vaporisation

Formation

Sublimation

0

1

2

3

A heating effect

No change in temperature

A cooling effect

Either (A) or (C)