Water
Air
Evaporative
Gas
B. Air
Fugacity
Partial pressure
Activity co-efficient
All (A), (B), and (C)
(T2 - T1)/T2
(T2 - T1)/T1
(T1 - T2)/T2
(T1 - T2)/T1
Molar concentration
Temperature
Internal energy
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
5 & 3
3.987 & 1.987
1.987 & 0.66
0.66 & 1.987
Cp of monatomic gases such as metallic vapor is about 5 kcal/kg.atom
The heat capacity of solid inorganic substance is exactly equal to the heat capacity of the substance in the molten state
There is an increase in entropy, when a spontaneous change occurs in an isolated system
At absolute zero temperature, the heat capacity for many pure crystalline substances is zero
n = y = 1.4
n = 0
n = 1
n = 1.66
Lowest
Highest
Average
None of these
Escaping tendencies of the same substance in different phases of a system
Relative volatility of a mixture of two miscible liquids
Behaviour of ideal gases
None of these
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
Reaction mechanism
Calculation of rates
Energy transformation from one form to another
None of these
Isothermal
Adiabatic
Isobaric
Isometric
Pressure
Temperature
Both (A) & (B)
Neither (A) nor (B)
H = E - PV
H = F - TS
H - E = PV
None of these
Cv.dT
Cp.dT
∫ Cp.dT
∫ Cv.dT
Enthalpy
Entropy
Pressure
None of these
Same as Carnot cycle
Same as reverse Carnot cycle
Dependent on the refrigerant's properties
The least efficient of all refrigeration processes
dE = CpdT
dE = CvdT
dQ = dE + pdV
dW = pdV
Entropy
Temperature
Internal energy
Enthalpy
If an insoluble gas is passed through a volatile liquid placed in a perfectly insulated container, the temperature of the liquid will increase
A process is irreversible as long as Δ S for the system is greater than zero
The mechanical work done by a system is always equal to∫P.dV
The heat of formation of a compound is defined as the heat of reaction leading to the formation of the compound from its reactants
Increase
Decrease
Remain unchanged
First fall and then rise
Internal energy
Enthalpy
Gibbs free energy
Helmholtz free energy
Increase the partial pressure of H2
Increase the partial pressure of I2
Increase the total pressure and hence shift the equilibrium towards the right
Not affect the equilibrium conditions
-1.87
0
1.26
3.91
Less than
Equal to
More than
Either (B) or (C); depends on the type of alloy
A heating effect
No change in temperature
A cooling effect
Either (A) or (C)
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
Melting point of ice
Melting point of wax
Boiling point of liquids
None of these
-2 RT ln 0.5
-RT ln 0.5
0.5 RT
2 RT
5.2
6.2
0.168
Data insufficient, can't be found out