Reversible and isothermal
Isothermal and irreversible
Reversible and adiabatic
Adiabatic and irreversible
C. Reversible and adiabatic
Molten sodium
Molten lead
Mercury
Molten potassium
Low temperature
High pressure
Both (A) and (B)
Neither (A) nor (B)
Two temperatures only
Pressure of working fluid
Mass of the working fluid
Mass and pressure both of the working fluid
A real gas on expansion in vacuum gets heated up
An ideal gas on expansion in vacuum gets cooled
An ideal gas on expansion in vacuum gets heated up
A real gas on expansion in vacuum cools down whereas ideal gas remains unaffected
-19.4
-30.2
55.2
-55.2
In which there is a temperature drop
Which is exemplified by a non-steady flow expansion
Which can be performed in a pipe with a constriction
In which there is an increase in temperature
Temperature
Mass
Volume
Pressure
Internal energy
Enthalpy
Gibbs free energy
Helmholtz free energy
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
2.73
28.3
273
283
0.15
1.5
4.5
6.5
Increases
Decreases
Remain same
Decreases linearly
Heating takes place
Cooling takes place
Pressure is constant
Temperature is constant
More
Less
Same
More or less; depending on the system
Isothermal
Adiabatic
Both (A) & (B)
Neither (A) nor (B)
Less than
More than
Same as
Not related to
300 × (32/7)
300 × (33/5)
300 × (333/7)
300 × (35/7)
The distribution law
Followed from Margules equation
A corollary of Henry's law
None of these
dQ = dE + dW
dQ = dE - dW
dE = dQ + dW
dW = dQ + dE
Entropy
Gibbs free energy
Internal energy
All (A), (B) & (C)
No heat and mass transfer
No mass transfer but heat transfer
Mass and energy transfer
None of these
Entropy
Gibbs energy
Internal energy
Enthalpy
Entropy
Internal energy
Enthalpy
Gibbs free energy
A gas may have more than one inversion temperatures
The inversion temperature is different for different gases
The inversion temperature is same for all gases
The inversion temperature is the temperature at which Joule-Thomson co-efficient is infinity
PV
2PV
PV/2
0
0
+ve
-ve
∞
Chemical potential
Surface tension
Heat capacity
None of these
Air cycle
Carnot cycle
Ordinary vapour compression cycle
Vapour compression with a reversible expansion engine
Less than
More than
Equal to or higher than
Less than or equal to
Maxwell's equation
Thermodynamic equation of state
Equation of state
Redlich-Kwong equation of state