Reversible isothermal volume change
Heating of a substance
Cooling of a substance
Simultaneous heating and expansion of an ideal gas
D. Simultaneous heating and expansion of an ideal gas
Same as Carnot cycle
Same as reverse Carnot cycle
Dependent on the refrigerant's properties
The least efficient of all refrigeration processes
0
2
1
3
Solution
Formation
Dilution
Combustion
High temperature
Low pressure
Low temperature only
Both low temperature and high pressure
Volume, mass and number of moles
Free energy, entropy and enthalpy
Both (A) and (B)
None of these
Adiabatic process
Endothermic reaction
Exothermic reaction
Process involving a chemical reaction
Virial co-efficients are universal constants
Virial co-efficients 'B' represents three body interactions
Virial co-efficients are function of temperature only
For some gases, Virial equations and ideal gas equations are the same
The conversion for a gas phase reaction increases with decrease in pressure, if there is an increase in volume accompanying the reaction
With increase in temperature, the equilibrium constant increases for an exothermic reaction
The equilibrium constant of a reaction depends upon temperature only
The conversion for a gas phase reaction increases with increase in pressure, if there is a decrease in volume accompanying the reaction
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)
Constant volume
Polytropic
Adiabatic
Constant pressure
Air cycle
Carnot cycle
Ordinary vapour compression cycle
Vapour compression with a reversible expansion engine
ΔF = ΔH + T [∂(ΔF)/∂T]P
ΔF = ΔH - TΔT
d(E - TS) T, V < 0
dP/dT = ΔHvap/T.ΔVvap
(∂P/∂V)T
(∂V/∂T)P
(∂P/∂V)V
All (A), (B) & (C)
TR/(T2 - TR) × (T1 - T2)/T1
TR/(T2 - TR) × T1/(T1 - T2)
TR/(T1 - TR) × (T1 - T2)/T1
None of these
CV
Enthalpy change
Free energy change
None of these
Direction of energy transfer
Reversible processes only
Irreversible processes only
None of these
(∂E/∂T)V
(∂E/∂V)T
(∂E/∂P)V
(∂V/∂T)P
Straight line
Sine curve
Parabola
Hyperbola
Momentum
Mass
Energy
None of these
Specific volume
Temperature
Mass
Pressure
Gibbs-Duhem
Van Laar
Gibbs-Helmholtz
Margules
Zero
Positive
Negative
None of these
A homogeneous solution (say of phenol water) is formed
Mutual solubility of the two liquids shows a decreasing trend
Two liquids are completely separated into two layers
None of these
Entropy
Gibbs free energy
Internal energy
All (A), (B) & (C)
Expansion of a real gas
Reversible isothermal volume change
Heating of an ideal gas
Cooling of a real gas
The expansion of a gas in vacuum is an irreversible process
An isometric process is a constant pressure process
Entropy change for a reversible adiabatic process is zero
Free energy change for a spontaneous process is negative
dE = Tds - PdV
dQ = CvdT + PdV
dQ = CpdT + Vdp
Tds = dE - PdV
None of these
Reversible isothermal
Irreversible isothermal
Reversible adiabatic
None of these
Simultaneous pressure & temperature change
Heating
Cooling
Both (B) and (C)