F = A + PV
F = E + A
F = A - TS
F = A + TS
A. F = A + PV
Internal energy
Enthalpy
Gibbs free energy
Helmholtz free energy
Use of only one graph for all gases
Covering of wide range
Easier plotting
More accurate plotting
More stable
Less stable
Not at all stable (like nascent O2)
Either more or less stable; depends on the compound
CV
Enthalpy change
Free energy change
None of these
Chemical potentials of a given component should be equal in all phases
Chemical potentials of all components should be same in a particular phase
Sum of the chemical potentials of any given component in all the phases should be the same
None of these
RT ln K
-RT ln K
-R ln K
T ln K
Isothermal
Adiabatic
Isentropic
None of these
Volume
Pressure
Temperature
All a, b & c
Steam to ethylene ratio
Temperature
Pressure
None of these
Two different gases behave similarly, if their reduced properties (i.e. P, V and T) are same
The surface of separation (i. e. the meniscus) between liquid and vapour phase disappears at the critical temperature
No gas can be liquefied above the critical temperature, howsoever high the pressure may be.
The molar heat of energy of gas at constant volume should be nearly constant (about 3 calories)
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
With pressure changes at constant temperature
Under reversible isothermal volume change
During heating of an ideal gas
During cooling of an ideal gas
Straight line
Sine curve
Parabola
Hyperbola
Only F decreases
Only A decreases
Both F and A decreases
Both F and A increase
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
72
92
142
192
At constant pressure, solubility of a gas in a liquid diminishes with rise in temperature
Normally, the gases which are easily liquefied are more soluble in common solvents
The gases which are capable of forming ions in aqueous solution are much more soluble in water than in other solvents
At constant pressure, solubility of a gas in a liquid increases with rise in temperature
Volume
Pressure
Temperature
All (A), (B) and (C)
Single phase fluid of varying composition
Single phase fluid of constant composition
Open as well as closed systems
Both (B) and (C)
Isometric
Polytropic
Isentropic
Isobaric
Pressure
Temperature
Composition
All (A), (B) and (C)
Pressure
Temperature
Both (A) & (B)
Neither (A) nor (B)
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
Adiabatic
Isometric
Isentropic
Isothermal
Non-flow reversible
Adiabatic
Both (A) and (B)
Neither (A) nor (B)
Less than
More than
Equal to or higher than
Less than or equal to
Volume
Temperature
Pressure
None of these
Superheated
Desuperheated
Non-condensable
None of these
Increases
Decreases
Remains unchanged
Decreases linearly
+ve
-ve
0
∞