Molal concentration difference

Molar free energy

Partial molar free energy

Molar free energy change

C. Partial molar free energy

Adiabatic process

Isothermal process

Isobaric process

All require same work

Latent heat of vaporisation

Chemical potential

Molal boiling point

Heat capacity

_{p}dT

_{v}dT

dQ = dE + pdV

dW = pdV

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

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

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

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

Like internal energy and enthalpy, the absolute value of standard entropy for elementary substances is zero

Melting of ice involves increase in enthalpy and a decrease in randomness

The internal energy of an ideal gas depends only on its pressure

Maximum work is done under reversible conditions

0

∞

+ve

-ve

A = H - TS

A = E - TS

A = H + TS

None of these

Pressure

Temperature

Volume

Molar concentration

Isothermal

Adiabatic

Isentropic

None of these

Not changed

Decreasing

Increasing

Data sufficient, can't be predicted

0

1

2

3

In an isothermal system, irreversible work is more than reversible work

Under reversible conditions, the adiabatic work is less than isothermal work

Heat, work, enthalpy and entropy are all 'state functions'

Matter and energy cannot be exchanged with the surroundings in a closed system

Isothermal

Adiabatic

Isentropic

Polytropic

Heating occurs

Cooling occurs

Pressure is constant

Temperature is constant

Sublimation

Vaporisation

Melting

Either (A), (B) or (C)

Pressure

Volume

Mass

None of these

Zero

Unity

Infinity

None of these

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

5 & 3

3.987 & 1.987

1.987 & 0.66

0.66 & 1.987

Specific volume

Temperature

Mass

Pressure

Isolated

Open

Insulated

Closed

_{2}

_{2}

Increase the total pressure and hence shift the equilibrium towards the right

Not affect the equilibrium conditions

Lewis-Randall

Margules

Van Laar

Both (B) & (C)

Increases

Decreases

Remains unchanged

Decreases linearly

Minimum

Zero

Maximum

None of these

Increase

Decrease

Remain unaltered

Increase or decrease; depends on the particular reaction

T = [RT/(V- b)] - [a/√T. V(V + b)]

^{2}) + ……

_{1}u_{2} + μ_{2}μ_{1} = 0

None of these

_{2}

_{3}

_{2}F_{2}

_{2}H_{4}Cl_{2}

Increases

Decreases

Remains unchanged

May increase or decrease; depends on the substance

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