x

x + 1

x + 2

x + 3

C. x + 2

Latent heat of vaporisation

Chemical potential

Molal boiling point

Heat capacity

Temperature

Mass

Volume

Pressure

At constant pressure

By throttling

By expansion in an engine

None of these

100,000 kW

160,000 kW

200,000 kW

320,000 kW

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

Enthalpies of all elements in their standard states are assumed to be zero

Combustion reactions are never endothermic in nature

Heat of reaction at constant volume is equal to the change in internal energy

Clausius-Clapeyron equation is not applicable to melting process

0

1

y = 1.44

1.66

Adiabatic

Isothermal

Isometric

None of these

Mole fraction

Activity

Pressure

Activity co-efficient

Entropy

Gibbs free energy

Internal energy

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

Use of only one graph for all gases

Covering of wide range

Easier plotting

More accurate plotting

P + F - C = 2

C = P - F + 2

F = C - P - 2

P = F - C - 2

^{Δx}, when Δx is negative

^{Δx}, when Δx is positive

Dimensionless, when Δx = 0

^{Δx2}, when Δx > 0

Independent of pressure

Independent of temperature

Zero at absolute zero temperature for a perfect crystalline substance

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

ΔF = ΔH + T [∂(ΔF)/∂T]P

ΔF = ΔH - TΔT

d(E - TS) T, V < 0

_{vap}/T.ΔV_{vap}

Adiabatic process

Isothermal process

Isobaric process

All require same work

Decrease in temperature

Increase in temperature

No change in temperature

Change in temperature which is a function of composition

Phase rule variables are intensive properties

Heat and work are both state function

The work done by expansion of a gas in vacuum is zero

_{P} and C_{V} are state function

0°C and 760 mm Hg

15°C and 760 mm Hg

20°C and 760 mm Hg

^{2}

349

651

667

1000

Joule-Thomson co-efficient

_{p})

co-efficient of thermal expansion

_{V})

Direction of energy transfer

Reversible processes only

Irreversible processes only

None of these

Volume

Pressure

Temperature

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

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

1.987 cal/gm mole °K

1.987 BTU/lb. mole °R

Both (A) and (B)

Neither (A) nor (B)

0.5

3.5

4.5

8.5

Zero

+ve

-ve

Dependent on the path

RT ln K

-RT ln K

-R ln K

T ln K

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

Adiabatic

Isothermal

Isometric

None of these