Sublimation
Vaporisation
Melting
Either (A), (B) or (C)
D. Either (A), (B) or (C)
Isothermal
Adiabatic
Isentropic
None of these
Volume, mass and number of moles
Free energy, entropy and enthalpy
Both (A) and (B)
None of these
Superheated
Desuperheated
Non-condensable
None of these
Free expansion of a gas
Compression of air in a compressor
Expansion of steam in a turbine
All (A), (B) & (C)
Surface tension
Free energy
Specific heat
Refractive index
Molten sodium
Molten lead
Mercury
Molten potassium
Adiabatic
Reversible
Isothermal
None of these
Adiabatic process
Endothermic reaction
Exothermic reaction
Process involving a chemical reaction
Solid-vapor
Solid-liquid
Liquid-vapor
All (A), (B) and (C)
0
1
∞
None of these
He
N2
O2
H2
Isothermal
Irreversible
Adiabatic
Reversible
Is the most efficient of all refrigeration cycles
Has very low efficiency
Requires relatively large quantities of air to achieve a significant amount of refrigeration
Both (B) and (C)
Lewis-Randall
Margules
Van Laar
Both (B) & (C)
μi = (∂F/∂ni)T, P, ni
μi = (∂A/∂ni)T, P, ni
μi = (∂F/∂ni)T, P
μi = (∂A/∂ni)T, P
Enthalpy
Volume
Both 'a' & 'b'
Neither 'a' nor 'b'
Molal concentration difference
Molar free energy
Partial molar free energy
Molar free energy change
1
< 1
> 1
>> 1
T = [RT/(V- b)] - [a/√T. V(V + b)]
PV/RT = 1 + (B/V) + (C/V2) + ……
n1u2 + μ2μ1 = 0
None of these
Low pressure and high temperature
Low pressure and low temperature
Low temperature and high pressure
High temperature and high pressure
Temperature
Pressure
Composition
All (A), (B) and (C)
Rate of heat transmission
Initial state only
End states only
None of these
Isobaric
Isothermal
Isentropic
Isometric
Kp2/Kp1 = - (ΔH/R) (1/T2 - 1/T1)
Kp2/Kp1 = (ΔH/R) (1/T2 - 1/T1)
Kp2/Kp1 = ΔH (1/T2 - 1/T1)
Kp2/Kp1 = - (1/R) (1/T2 - 1/T1)
Surface tension of a substance vanishes at critical point, as there is no distinction between liquid and vapour phases at its critical point
Entropy of a system decreases with the evolution of heat
Change of internal energy is negative for exothermic reactions
The eccentric factor for all materials is always more than one
In an isothermal system, irreversible work is more than reversible work
Under reversible conditions, the adiabatic work is less than isothermal work
Heat, work, enthalpy and entropy are all 'state functions'
Matter and energy cannot be exchanged with the surroundings in a closed system
4 J
∞
0
8 J
Volume of the liquid phase is negligible compared to that of vapour phase
Vapour phase behaves as an ideal gas
Heat of vaporisation is independent of temperature
All (A), (B) & (C)
Isothermally
Isobarically
Adiabatically
None of these
Heat capacity of a crystalline solid is zero at absolute zero temperature
Heat transfer from low temperature to high temperature source is not possible without external work
Gases having same reduced properties behaves similarly
None of these