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

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

Decreases

Increases

Remain same

Decreases linearly

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

The statement as per Gibbs-Helmholtz

Called Lewis-Randall rule

Henry's law

None of these

0

273

25

None of these

Non-flow reversible

Adiabatic

Both (A) and (B)

Neither (A) nor (B)

Molecular size

Volume

Pressure

Temperature

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

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

_{1}/T_{2}

_{2}/R_{1}

_{1}ACBP_{2}P_{1}

^{1}A^{1}A

ACBDA

^{1}A^{1}A

-1.87

0

1.26

3.91

Amount of energy transferred

Direction of energy transfer

Irreversible processes only

Non-cyclic processes only

Turbine

Heat engine

Reversed heat engine

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

At constant pressure

By throttling

By expansion in an engine

None of these

Adiabatic process

Isothermal process

Isobaric process

All require same work

Moisture free ice

Solid helium

Solid carbon dioxide

None of these

Vapor pressure

Specific Gibbs free energy

Specific entropy

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

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

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

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

None of these

Mass

Momentum

Energy

None of these

Bertholet equation

Clausius-Clapeyron equation

Beattie-Bridgeman equation

None of these

Increase

Decrease

No change

None of these

Same

Doubled

Halved

One fourth of its original value

Rate of change of vapour pressure with temperature

Effect of an inert gas on vapour pressure

Calculation of ΔF for spontaneous phase change

Temperature dependence of heat of phase transition

Zero

One

Infinity

Negative

2.73

28.3

273

283

J/s

J.S

J/kmol

kmol/J

Entropy

Temperature

Internal energy

Enthalpy

Does not depend upon temperature

Is independent of pressure only

Is independent of volume only

Is independent of both pressure and volume

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

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

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

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

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

Snow melts into water

A gas expands spontaneously from high pressure to low pressure

Water is converted into ice

Both (B) & (C)