_{S} = (∂P/∂V)_{T}

_{S} = [(∂P/∂V)_{T}]^{Y}

_{S} = y(∂P/∂V)_{T}

_{S} = 1/y(∂P/∂V)_{T}

C. (∂P/∂V)_{S} = y(∂P/∂V)_{T}

Volume

Mass

Critical temperature

None of these

Reversible and isothermal

Irreversible and constant enthalpy

Reversible and constant entropy

Reversible and constant enthalpy

_{p} < C_{v}

_{p} = C_{v}

_{p} > C_{v}

_{v}

Zeroth

First

Second

Third

Temperature

Mass

Volume

Pressure

Increases

Decreases

Remain same

Decreases linearly

No

Any real

Only ideal

Both (B) and (C)

5.2

6.2

0.168

Data insufficient, can't be found out

Initial concentration of the reactant

Pressure

Temperature

None of these

0

1

2

3

RT d ln P

RT d ln f

R d ln f

None of these

Air cycle

Carnot cycle

Ordinary vapour compression cycle

Vapour compression with a reversible expansion engine

Two isothermal and two isentropic

Two isobaric and two isothermal

Two isochoric and two isobaric

Two isothermals and two isochoric

-94 kcal

> -94 kcal

< - 94 kcal

Zero

Vapour pressure is relatively low and the temperature does not vary over wide limits

Vapour obeys the ideal gas law and the latent heat of vaporisation is constant

Volume in the liquid state is negligible compared with that in the vapour state

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

Less pronounced

More pronounced

Equal

Data insufficient, can't be predicted

Departure from ideal solution behaviour

Departure of gas phase from ideal gas law

Vapour pressure of liquid

None of these

Straight line

Sine curve

Parabola

Hyperbola

More stable

Less stable

Not at all stable (like nascent O2)

Either more or less stable; depends on the compound

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

Le-Chatelier principle

Kopp's rule

Law of corresponding state

Arrhenius hypothesis

Increases

Decreases

Remains unchanged

Decreases linearly

Only enthalpy change (ΔH) is negative

Only internal energy change (ΔE) is negative

Both ΔH and ΔE are negative

Enthalpy change is zero

Specific volume

Work

Pressure

Temperature

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

Water

Air

Evaporative

Gas

Ideal compression of air

Free expansion of an ideal gas

Adiabatic expansion of steam in a turbine

Adiabatic compression of a perfect gas

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

More

Less

Same

Unpredictable; depends on the particular reaction

448

224

22.4

Data insufficient; can't be computed