The same

Less than

Greater than

Different than

A. The same

Helmholtz

Gibbs

Both a & b

Neither 'a' nor 'b'

PV

2PV

PV/2

0

Use of only one graph for all gases

Covering of wide range

Easier plotting

More accurate plotting

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

Increase

Decrease

Remain unchanged

First fall and then rise

Specific volume

Temperature

Mass

Pressure

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

Two temperatures only

Pressure of working fluid

Mass of the working fluid

Mass and pressure both of the working fluid

Negative

Zero

Infinity

None of these

Saturated vapour

Solid

Gas

Liquid

Minimum number of degree of freedom of a system is zero

Degree of freedom of a system containing a gaseous mixture of helium, carbon dioxide and hydrogen is 4

For a two phase system in equilibrium made up of four non-reacting chemical species, the number of degrees of freedom is 4

Enthalpy and internal energy change is zero during phase change processes like melting, vaporisation and sublimation

State functions

Path functions

Intensive properties

Extensive properties

ds = 0

ds < 0

ds > 0

ds = Constant

A closed system does not permit exchange of mass with its surroundings but may permit exchange of energy.

An open system permits exchange of both mass and energy with its surroundings

The term microstate is used to characterise an individual, whereas macro-state is used to designate a group of micro-states with common characteristics

None of the above

6738.9

6753.5

7058.3

9000

Non-flow reversible

Adiabatic

Both (A) and (B)

Neither (A) nor (B)

0°C and 750 mm Hg

15°C and 750 mm Hg

0°C and 1 kgf/cm2

15°C and 1 kgf/cm2

0

+ve

-ve

∞

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'

30554

10373

4988.4

4364.9

The amount of work needed is path dependent

Work alone cannot bring out such a change of state

The amount of work needed is independent of path

More information is needed to conclude anything about the path dependence or otherwise of the work needed

Becomes zero

Becomes infinity

Equals 1 kcal/kmol °K

Equals 0.24 kcal/kmol °K

4 J

∞

0

8 J

Zero

Unity

Infinity

Negative

Decreases

Increases

Remain same

Decreases linearly

Non-uniformly

Adiabatically

Isobarically

Isothermally

Only F decreases

Only A decreases

Both F and A decreases

Both F and A increase

Entropy

Gibbs free energy

Internal energy

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

Reaction mechanism

Calculation of rates

Energy transformation from one form to another

None of these

Increases with rise in pressure

Decreases with rise in pressure

Is independent of pressure

Is a path function