Temperature
Pressure
Volume
Entropy
B. Pressure
(∂T/∂V)S = (∂p/∂S)V
(∂T/∂P)S = (∂V/∂S)P
(∂P/∂T)V = (∂S/∂V)T
(∂V/∂T)P = -(∂S/∂P)T
Phase rule variables are intensive properties
Heat and work are both state function
The work done by expansion of a gas in vacuum is zero
CP and CV are state function
Temperature vs. enthalpy
Temperature vs. enthalpy
Entropy vs. enthalpy
Temperature vs. internal energy
n = y = 1.4
n = 0
n = 1
n = 1.66
Increases
Decreases
Remain constant
Increases linearly
Zero
One
Infinity
Negative
Is the analog of linear frictionless motion in machines
Is an idealised visualisation of behaviour of a system
Yields the maximum amount of work
Yields an amount of work less than that of a reversible process
Isothermal
Isobaric
Polytropic
Adiabatic
More
Less
Same
More or less; depending on the system
< 0
> 0
= 0
None of these
Reversible isothermal
Irreversible isothermal
Reversible adiabatic
None of these
The concentration of each component should be same in the two phases
The temperature of each phase should be same
The pressure should be same in the two phases
The chemical potential of each component should be same in the two phases
A refrigeration cycle violates the second law of thermodynamics
Refrigeration cycle is normally represented by a temperature vs. entropy plot
In a refrigerator, work required decreases as the temperature of the refrigerator and the temperature at which heat is rejected increases
One ton of refrigeration is equivalent to the rate of heat absorption equal to 3.53 kW
0
1
y = 1.44
1.66
Increased COP
Same COP
Decreased COP
Increased or decreased COP; depending upon the type of refrigerant
At low temperature and high pressure
At standard state
Both (A) and (B)
In ideal state
0
1
2
3
∞
-ve
0
+ve
(∂E/∂T)V
(∂E/∂V)T
(∂E/∂P)V
(∂V/∂T)P
+ve
-ve
0
Either of the above three; depends on the nature of refrigerant
Critical
Boyle
Inversion
Reduced
T
√T
T2
1/√T
Critical temperature
Melting point
Freezing point
Both (B) and (C)
50 kcal/hr
200 BTU/hr
200 BTU/minute
200 BTU/day
Latent heat of vaporisation
Chemical potential
Molal boiling point
Heat capacity
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
Expansion in an engine
Following a constant pressure cycle
Throttling
None of these
Joule-Thomson co-efficient
Specific heat at constant pressure (Cp)
co-efficient of thermal expansion
Specific heat at constant volume (CV)
Activity
Fugacity
Activity co-efficient
Fugacity co-efficient
Closed
Open
Isolated
Non-thermodynamic