Less
More
Same
Dependent on climatic conditions
A. Less
1
2
3
4
Minimum
Zero
Maximum
None of these
Freezing
Triple
Boiling
Boyle
dQ = dE + dW
dQ = dE - dW
dE = dQ + dW
dW = dQ + dE
Activity co-efficient is dimensionless.
In case of an ideal gas, the fugacity is equal to its pressure.
In a mixture of ideal gases, the fugacity of a component is equal to the partial pressure of the component.
The fugacity co-efficient is zero for an ideal gas
(∂E/∂ni)S, v, nj
(∂G/∂ni)T, P, nj = (∂A/∂ni) T, v, nj
(∂H/∂ni)S, P, nj
All (A), (B) and (C)
Does not depend upon temperature
Is independent of pressure only
Is independent of volume only
Is independent of both pressure and volume
Zeroth
First
Second
Third
P + F - C = 2
C = P - F + 2
F = C - P - 2
P = F - C - 2
100
50
205
200
The available energy in an isolated system for all irreversible (real) processes decreases
The efficiency of a Carnot engine increases, if the sink temperature is decreased
The reversible work for compression in non-flow process under isothermal condition is the change in Helmholtz free energy
All (A), (B) and (C)
Isothermal
Adiabatic
Isobaric
Isochoric
300 × (32/7)
300 × (33/5)
300 × (333/7)
300 × (35/7)
An ideal liquid or solid solution is defined as one in which each component obeys Raoult's law
If Raoult's law is applied to one component of a binary mixture; Henry's law or Raoult's law is applied to the other component also
Henry's law is rigorously correct in the limit of infinite dilution
None of these
Surface tension
Free energy
Specific heat
Refractive index
Decrease in velocity
Decrease in temperature
Decrease in kinetic energy
Energy spent in doing work
RT ln K
-RT ln K
-R ln K
T ln K
Reversible isothermal volume change
Heating of a substance
Cooling of a substance
Simultaneous heating and expansion of an ideal gas
Compressibility
Work done under adiabatic condition
Work done under isothermal condition
Co-efficient of thermal expansion
Reversible and isothermal
Irreversible and constant enthalpy
Reversible and constant entropy
Reversible and constant enthalpy
Pressure
Temperature
Both (A) & (B)
Neither (A) nor (B)
Critical
Triple
Freezing
Boiling
Decrease on addition of Cl2
Increase on addition of an inert gas at constant pressure
Decrease on increasing the pressure of the system
None of these
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
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
Two temperatures only
Pressure of working fluid
Mass of the working fluid
Mass and pressure both of the working fluid
Violates second law of thermodynamics
Involves transfer of heat from low temperature to high temperature
Both (A) and (B)
Neither (A) nor (B)
Less than
More than
Equal to or higher than
Less than or equal to
μi = (∂F/∂ni)T, P, ni
μi = (∂A/∂ni)T, P, ni
μi = (∂F/∂ni)T, P
μi = (∂A/∂ni)T, P
Carnot
Air
Absorption
vapour-ejection