0
2
1
3
C. 1
The net change in entropy in any reversible cycle is always zero
The entropy of the system as a whole in an irreversible process increases
The entropy of the universe tends to a maximum
The entropy of a substance does not remain constant during a reversible adiabatic change
Water
Air
Evaporative
Gas
Two temperatures only
Pressure of working fluid
Mass of the working fluid
Mass and pressure both of the working fluid
ΔF = ΔH + T [∂(ΔF)/∂T]P
ΔF = ΔH - TΔT
d(E - TS) T, V < 0
dP/dT = ΔHvap/T.ΔVvap
Temperature
Pressure
Composition
All (A), (B) and (C)
Volume
Temperature
Pressure
None of these
Reversible
Irreversible
Isothermal
Adiabatic
Heat pump
Heat engine
Carnot engine
None of these
Solution
Formation
Dilution
Combustion
Triple point
Boiling point
Below triple point
Always
With pressure changes at constant temperature
Under reversible isothermal volume change
During heating of an ideal gas
During cooling of an ideal gas
Two isothermal and two isentropic
Two isobaric and two isothermal
Two isochoric and two isobaric
Two isothermals and two isochoric
Heat capacity
Molal heat capacity
Pressure
Concentration
Not changed
Decreasing
Increasing
Data sufficient, can't be predicted
Reaction mechanism
Calculation of rates
Energy transformation from one form to another
None of these
Vapour pressure is relatively low and the temperature does not vary over wide limits
Vapour obeys the ideal gas law and the latent heat of vaporisation is constant
Volume in the liquid state is negligible compared with that in the vapour state
All (A), (B) and (C)
Kelvin's
Antoines
Kirchoffs
None of these
Joule-Thomson co-efficient
Specific heat at constant pressure (Cp)
co-efficient of thermal expansion
Specific heat at constant volume (CV)
Activity co-efficient is dimensionless.
In case of an ideal gas, the fugacity is equal to its pressure.
In a mixture of ideal gases, the fugacity of a component is equal to the partial pressure of the component.
The fugacity co-efficient is zero for an ideal gas
Concentration of the constituents only
Quantities of the constituents only
Temperature only
All (A), (B) and (C)
Pressure
Temperature
Volume
Molar concentration
0
> 0
< 0
None of these
-2 RT ln 0.5
-RT ln 0.5
0.5 RT
2 RT
Addition of inert gas favours the forward reaction, when Δx is positive
Pressure has no effect on equilibrium, when Δn = 0
Addition of inert gas has no effect on the equilibrium constant at constant volume for any value of Δx (+ ve, - ve) or zero)
All 'a', 'b' & 'c'
Equilibrium cannot be established
More ice will be formed
More water will be formed
Evaporation of water will take place
Violates second law of thermodynamics
Involves transfer of heat from low temperature to high temperature
Both (A) and (B)
Neither (A) nor (B)
Increases
Decreases
Remains unchanged
May increase or decrease; depends on the substance
12 P1V1
6 P1 V1
3 P1V1
P1 V1
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
Entropy
Gibbs energy
Internal energy
Enthalpy