Only F decreases

Only A decreases

Both F and A decreases

Both F and A increase

C. Both F and A decreases

Gibbs-Duhem equation

Gibbs-Helmholtz equation

Third law of thermodynamics

Joule-Thomson effect

Minimum

Zero

Maximum

None of these

P + F - C = 2

C = P - F + 2

F = C - P - 2

P = F - C - 2

Number of intermediate chemical reactions involved

Pressure and temperature

State of combination and aggregation in the beginning and at the end of the reaction

None of these

_{V}

Enthalpy change

Free energy change

None of these

∞

+ve

0

-ve

Tds = dE - dW = 0

dE - dW - Tds = 0

Tds - dE + dW < 0

Tds - dT + dW < 0

Specific volume

Temperature

Mass

Pressure

In standard state

At high pressure

At low temperature

In ideal state

Work done under adiabatic condition

Co-efficient of thermal expansion

Compressibility

None of these

Enthalpy

Entropy

Pressure

None of these

An ideal liquid or solid solution is defined as one in which each component obeys Raoult's law

If Raoult's law is applied to one component of a binary mixture; Henry's law or Raoult's law is applied to the other component also

Henry's law is rigorously correct in the limit of infinite dilution

None of these

Maxwell's equation

Clausius-Clapeyron Equation

Van Laar equation

Nernst Heat Theorem

Reaction mechanism

Calculation of rates

Energy transformation from one form to another

None of these

Simultaneous pressure & temperature change

Heating

Cooling

Both (B) and (C)

Equilibrium

Adiabatic

Steady

Unsteady

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

Solubility increases as temperature increases

Solubility increases as temperature decreases

Solubility is independent of temperature

Solubility increases or decreases with temperature depending on the Gibbs free energy change of solution

Le-Chatelier principle

Kopp's rule

Law of corresponding state

Arrhenius hypothesis

Zero

One

Two

Three

_{S} = (∂p/∂S)_{V}

_{S} = (∂V/∂S)_{P}

_{V} = (∂S/∂V)_{T}

_{P} = -(∂S/∂P)_{T}

Temperature

Pressure

Composition

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

its internal energy (U) decreases and its entropy (S) increases

U and S both decreases

U decreases but S is constant

U is constant but S decreases

Increases

Decreases

Remains unchanged

Decreases linearly

Entropy

Temperature

Internal energy

Enthalpy

0.5

3.5

4.5

8.5

V/T = Constant

V ∝ 1/T

V ∝ 1/P

PV/T = Constant

Only ΔE = 0

Only ΔH =0

ΔE = ΔH = 0

dQ = dE

Sublimation

Vaporisation

Melting

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

Heat capacity

Molal heat capacity

Pressure

Concentration