Always greater than one
Same at the same reduced temperature
Same at the same reduced pressure
Both (B) & (C)
D. Both (B) & (C)
√(2KT/m)
√(3KT/m)
√(6KT/m)
3KT/m
Pressure and temperature
Reduced pressure and reduced temperature
Critical pressure and critical temperature
None of these
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
Gibbs-Duhem equation
Gibbs-Helmholtz equation
Third law of thermodynamics
Joule-Thomson effect
Enthalpy
Internal energy
Either (A) or (B)
Neither (A) nor (B)
Isobaric
Adiabatic
Isenthalpic
Both (B) & (C)
Δ S1 is always < Δ SR
Δ S1 is sometimes > Δ SR
Δ S1 is always > Δ SR
Δ S1 is always = Δ SR
5 & 3
3.987 & 1.987
1.987 & 0.66
0.66 & 1.987
Addition of inert gas favours the forward reaction, when Δx is positive
Pressure has no effect on equilibrium, when Δn = 0
Addition of inert gas has no effect on the equilibrium constant at constant volume for any value of Δx (+ ve, - ve) or zero)
All 'a', 'b' & 'c'
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
Zeroth
First
Second
Third
Low pressure and high temperature
Low pressure and low temperature
High pressure and low temperature
High pressure and high temperature
-273
0
-78
5
0
< 0
< 1
> 1
Molecular size
Volume
Pressure
Temperature
Infinity
Minus infinity
Zero
None of these
Both the processes are adiabatic
Both the processes are isothermal
Process A is isothermal while B is adiabatic
Process A is adiabatic while B is isothermal
Only F decreases
Only A decreases
Both F and A decreases
Both F and A increase
Entropy and enthalpy are path functions
In a closed system, the energy can be exchanged with the surrounding, while matter cannot be exchanged
All the natural processes are reversible in nature
Work is a state function
Zeroth
First
Second
Third
CV
Entropy change
Gibbs free energy
None of these
Hess's
Kirchoff's
Lavoisier and Laplace
None of these
Momentum
Mass
Energy
None of these
Low pressure and high temperature
Low pressure and low temperature
Low temperature and high pressure
High temperature and high pressure
Use of only one graph for all gases
Covering of wide range
Easier plotting
More accurate plotting
(atm)Δx, when Δx is negative
(atm)Δx, when Δx is positive
Dimensionless, when Δx = 0
(atm)Δx2, when Δx > 0
Expansion of an ideal gas against constant pressure
Atmospheric pressure vaporisation of water at 100°C
Solution of NaCl in water at 50°C
None of these
Solution
Vaporisation
Formation
Sublimation
0
1
2
3
A heating effect
No change in temperature
A cooling effect
Either (A) or (C)