Independent of pressure
Independent of temperature
Zero at absolute zero temperature for a perfect crystalline substance
All (A), (B) & (C)
Specific volume
Work
Pressure
Temperature
Zero
Negative
Very large compared to that for endothermic reaction
Not possible to predict
Departure from ideal solution behaviour
Departure of gas phase from ideal gas law
Vapour pressure of liquid
None of these
Isochoric
Isobaric
Adiabatic
Isothermal
Equilibrium cannot be established
More ice will be formed
More water will be formed
Evaporation of water will take place
Less
More
Same
More or less depending upon the extent of work done
Pressure
Solubility
Temperature
None of these
Air cycle
Carnot cycle
Ordinary vapor compression cycle
Vapor compression with a reversible expansion engine
448
224
22.4
Data insufficient; can't be computed
Direction of energy transfer
Reversible processes only
Irreversible processes only
None of these
Path
Point
State
None of these
Increase the partial pressure of H2
Increase the partial pressure of I2
Increase the total pressure and hence shift the equilibrium towards the right
Not affect the equilibrium conditions
∞
1
0
-ve
In an isothermal system, irreversible work is more than reversible work
Under reversible conditions, the adiabatic work is less than isothermal work
Heat, work, enthalpy and entropy are all 'state functions'
Matter and energy cannot be exchanged with the surroundings in a closed system
Minimum number of degree of freedom of a system is zero
Degree of freedom of a system containing a gaseous mixture of helium, carbon dioxide and hydrogen is 4
For a two phase system in equilibrium made up of four non-reacting chemical species, the number of degrees of freedom is 4
Enthalpy and internal energy change is zero during phase change processes like melting, vaporisation and sublimation
Gibbs-Duhem
Maxwell's
Clapeyron
None of these
Zero
Unity
Infinity
None of these
0
1
2
3
Solids
Liquids
Gases
All (A), (B) & (C)
Number of intermediate chemical reactions involved
Pressure and temperature
State of combination and aggregation in the beginning and at the end of the reaction
None of these
Enhanced COP
Decreased COP
No change in the value of COP
Increased or decreased COP; depending upon the type of refrigerant
Low temperature
High pressure
Both (A) and (B)
Neither (A) nor (B)
T1/(T1-T2)
T2/(T1-T2)
T1/T2
T2/R1
Compressibility
Work done under adiabatic condition
Work done under isothermal condition
Co-efficient of thermal expansion
The amount of work needed is path dependent
Work alone cannot bring out such a change of state
The amount of work needed is independent of path
More information is needed to conclude anything about the path dependence or otherwise of the work needed
Use of only one graph for all gases
Covering of wide range
Easier plotting
More accurate plotting
dE = CpdT
dE = CvdT
dQ = dE + pdV
dW = pdV
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
Does not depend upon temperature
Is independent of pressure only
Is independent of volume only
Is independent of both pressure and volume