Cv.dT
Cp.dT
∫ Cp.dT
∫ Cv.dT
C. ∫ Cp.dT
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
Increase
Decrease
Remain unchanged
First fall and then rise
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
Turbine
Heat engine
Reversed heat engine
None of these
Heating takes place
Cooling takes place
Pressure is constant
Temperature is constant
Triple point
Boiling point
Below triple point
Always
Temperature
Specific heat
Volume
Pressure
3
4
5
6
Increases
Decreases
Remain constant
Increases linearly
0
1
2
3
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
T
√T
T2
1/√T
System and surroundings pressure be equal
Friction in the system should be absent
System and surroundings temperature be equal
None of these
Like internal energy and enthalpy, the absolute value of standard entropy for elementary substances is zero
Melting of ice involves increase in enthalpy and a decrease in randomness
The internal energy of an ideal gas depends only on its pressure
Maximum work is done under reversible conditions
Cv.dT
Cp.dT
∫ Cp.dT
∫ Cv.dT
Pressure
Volume
Mass
None of these
2
0
3
1
Not a function of its pressure
Not a function of its nature
Not a function of its temperature
Unity, if it follows PV = nRT
580
640
1160
Data insufficient; can't be computed
Increases, for an exothermic reaction
Decreases, for an exothermic reaction
Increases, for an endothermic reaction
None of these
Gibbs-Duhem equation
Gibbs-Helmholtz equation
Third law of thermodynamics
Joule-Thomson effect
Increases
Decreases
Remains unchanged
Decreases linearly
Cp < Cv
Cp = Cv
Cp > Cv
C ≥ Cv
Entropy
Gibbs free energy
Internal energy
All (A), (B) & (C)
Activity
Fugacity
Activity co-efficient
Fugacity co-efficient
Two
One
Zero
Three
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
No
Any real
Only ideal
Both (B) and (C)
Enthalpy
Pressure
Entropy
None of these
0
1
2
3