Isothermal
Adiabatic
Isentropic
None of these
A. Isothermal
Equilibrium cannot be established
More ice will be formed
More water will be formed
Evaporation of water will take place
Cp < Cv
Cp = Cv
Cp > Cv
C ≥ Cv
0
∞
+ ve
- ve
Zero
Positive
Negative
None of these
Momentum
Mass
Energy
None of these
dE = Tds - PdV
dQ = CvdT + PdV
dQ = CpdT + Vdp
Tds = dE - PdV
Entropy
Gibbs free energy
Internal energy
All (A), (B) & (C)
Only enthalpy change (ΔH) is negative
Only internal energy change (ΔE) is negative
Both ΔH and ΔE are negative
Enthalpy change is zero
Increases
Decreases
Remains unchanged
First decreases and then increases
Molar concentration
Temperature
Internal energy
None of these
Minimum
Zero
Maximum
Indeterminate
Chemical potential
Surface tension
Heat capacity
None of these
Shifting the equilibrium towards right
Shifting the equilibrium towards left
No change in equilibrium condition
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)
The statement as per Gibbs-Helmholtz
Called Lewis-Randall rule
Henry's law
None of these
Not have a sub-atmospheric vapour pressure at the temperature in the refrigerator coils
Not have unduly high vapour pressure at the condenser temperature
Both (A) and (B)
Have low specific heat
Fugacity
Partial pressure
Activity co-efficient
All (A), (B), and (C)
Volume, mass and number of moles
Free energy, entropy and enthalpy
Both (A) and (B)
None of these
Increases
Decreases
Remain constant
Increases linearly
Isothermal
Adiabatic
Both (A) & (B)
Neither (A) nor (B)
Steam engine
Carnot engine
Diesel engine
Otto engine
The surface tension vanishes
Liquid and vapour have the same density
There is no distinction between liquid and vapour phases
All (A), (B) and (C)
Adiabatic
Isothermal
Isometric
None of these
0
∞
50
100
μ° + RT ln f
μ°+ R ln f
μ° + T ln f
μ° + R/T ln f
0
< 0
< 1
> 1
270
327
300
540
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
The chemical potential of ith species (μi) in an ideal gas mixture approaches zero as the pressure or mole fraction (xi) tends to be zero at constant temperature
The chemical potential of species 'i' in the mixture (μi) is mathematically represented as,μi = ∂(nG)/∂ni]T,P,nj where, n, ni and nj respectively denote the total number of moles, moles of ith species and all mole numbers except ith species. 'G' is Gibbs molar free energy
An open system of constant composition
A closed system of constant composition
An open system with changes in composition
A closed system with changes in composition
CV
Entropy change
Gibbs free energy
None of these