Equal to its density

The reciprocal of its density

Proportional to pressure

None of these

B. The reciprocal of its density

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

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

_{1}/T_{2}

_{2}/R_{1}

Internal energy

Enthalpy

Entropy

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

∞

0

< 0

> 0

1.572

1.9398

3.389

4.238

1

2

3

4

0

273

25

None of these

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

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

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

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

Adiabatic

Isothermal

Isometric

None of these

_{2}

_{2}

_{2}

_{2}

Decreases

Increases

Remains constant

Decreases logarithmically

Always greater than one

Same at the same reduced temperature

Same at the same reduced pressure

Both (B) & (C)

A homogeneous solution (say of phenol water) is formed

Mutual solubility of the two liquids shows a decreasing trend

Two liquids are completely separated into two layers

None of these

Independent of pressure

Independent of temperature

Zero at absolute zero temperature for a perfect crystalline substance

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

0

1

2

3

Vapor pressure

Partial pressure

Chemical potential

None of these

No

Any real

Only ideal

Both (B) and (C)

The chemical potential of a pure substance depends upon the temperature and pressure

The chemical potential of a component in a system is directly proportional to the escaping tendency of that component

_{i}) in an ideal gas mixture approaches zero as the pressure or mole fraction (x_{i}) tends to be zero at constant temperature

_{i}) is mathematically represented as,μ_{i} = ∂(nG)/∂ni]_{T,P,nj} where, n, n_{i} and n_{j} respectively denote the total number of moles, moles of i^{th} species and all mole numbers except ith species. 'G' is Gibbs molar free energy

3

2

1

0

Water

Air

Evaporative

Gas

Bertholet equation

Clausius-Clapeyron equation

Beattie-Bridgeman equation

None of these

P ∝ 1/V, when temperature is constant

P ∝ 1/V, when temperature & mass of the gas remain constant

P ∝ V, at constant temperature & mass of the gas

P/V = constant, for any gas

5.2

6.2

0.168

Data insufficient, can't be found out

_{2}/Kp_{1} = - (ΔH/R) (1/T_{2} - 1/T_{1})

_{2}/Kp_{1} = (ΔH/R) (1/T_{2} - 1/T_{1})

_{2}/Kp_{1} = ΔH (1/T_{2} - 1/T_{1})

_{2}/Kp_{1} = - (1/R) (1/T_{2} - 1/T_{1})

State functions

Path functions

Intensive properties

Extensive properties

Triple point

Boiling point

Below triple point

Always

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

Accomplishes only space heating in winter

Accomplishes only space cooling in summer

Accomplishes both (A) and (B)

Works on Carnot cycle

Fusion

Vaporisation

Transition

None of these

_{V}

_{T}

_{V}

_{P}

-94 kcal

> -94 kcal

< - 94 kcal

Zero