Same as Carnot cycle

Same as reverse Carnot cycle

Dependent on the refrigerant's properties

The least efficient of all refrigeration processes

B. Same as reverse Carnot cycle

ΔF = ΔH + T [∂(ΔF)/∂T]P

ΔF = ΔH - TΔT

d(E - TS) T, V < 0

_{vap}/T.ΔV_{vap}

Entropy

Gibbs energy

Internal energy

Enthalpy

Molal concentration difference

Molar free energy

Partial molar free energy

Molar free energy change

Reversible and isothermal

Irreversible and constant enthalpy

Reversible and constant entropy

Reversible and constant enthalpy

Reversible isothermal

Irreversible isothermal

Reversible adiabatic

None of these

Volume of the liquid phase is negligible compared to that of vapour phase

Vapour phase behaves as an ideal gas

Heat of vaporisation is independent of temperature

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

Logarithmic

Arithmetic

Geometric

Harmonic

Same in both the phases

Zero in both the phases

More in vapour phase

More in liquid phase

Is the analog of linear frictionless motion in machines

Is an idealised visualisation of behaviour of a system

Yields the maximum amount of work

Yields an amount of work less than that of a reversible process

Solution

Vaporisation

Formation

Sublimation

0

1

y = 1.44

1.66

Expansion of a real gas

Reversible isothermal volume change

Heating of an ideal gas

Cooling of a real gas

_{1} - 1/T_{2})

_{1} - 1/T_{2})

_{2} - 1/T_{1})

_{1} - 1/T_{2})

Closed

Open

Isolated

Non-thermodynamic

Vant-Hoff equation

Le-Chatelier's principle

Arrhenius equation

None of these

5 & 3

3.987 & 1.987

1.987 & 0.66

0.66 & 1.987

Isobaric

Isothermal

Isentropic

Isometric

0

> 0

< 0

None of these

Endothermic

Exothermic

Isothermal

Adiabatic

Only enthalpy change (ΔH) is negative

Only internal energy change (ΔE) is negative

Both ΔH and ΔE are negative

Enthalpy change is zero

RT ln K

-RT ln K

-R ln K

T ln K

Molecular size

Volume

Pressure

Temperature

State function

Macroscopic property

Extensive property

None of these

0

1

2

3

Are more or less constant (vary from 0.2 to 0.3)

Vary as square of the absolute temperature

Vary as square of the absolute pressure

None of these

The statement as per Gibbs-Helmholtz

Called Lewis-Randall rule

Henry's law

None of these

Heat capacity of a crystalline solid is zero at absolute zero temperature

Heat transfer from low temperature to high temperature source is not possible without external work

Gases having same reduced properties behaves similarly

None of these

Δ H = 0 and ΔS = 0

Δ H ≠ 0 and ΔS = 0

Δ H ≠ 0 and ΔS ≠ 0

Δ H = 0 and ΔS ≠ 0

Volume

Enthalpy

Both (A) & (B)

Neither (A) nor (B)

More

Less

Same

More or less; depending on the system