Process must be isobaric
Temperature must decrease
Process must be adiabatic
Both (B) and (C)
D. Both (B) and (C)
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
State functions
Path functions
Intensive properties
Extensive properties
Low temperature
High pressure
Both (A) and (B)
Neither (A) nor (B)
Temperature
Pressure
Volume
None of these
More stable
Less stable
Not at all stable (like nascent O2)
Either more or less stable; depends on the compound
Steam engine
Carnot engine
Diesel engine
Otto engine
A . x22
Ax1
Ax2
Ax12
Increases
Decreases
Remains unchanged
First decreases and then increases
Entropy
Internal energy
Enthalpy
Gibbs free energy
At constant pressure
By throttling
By expansion in an engine
None of these
Molecular size
Temperature
Volume
Pressure
Lewis-Randall
Margules
Van Laar
Both (B) & (C)
Reaction mechanism
Calculation of rates
Energy transformation from one form to another
None of these
Decreases
Increases
Remains constant
Decreases logarithmically
Activity
Fugacity
Activity co-efficient
Fugacity co-efficient
(∂P/∂V)S = (∂P/∂V)T
(∂P/∂V)S = [(∂P/∂V)T]Y
(∂P/∂V)S = y(∂P/∂V)T
(∂P/∂V)S = 1/y(∂P/∂V)T
Water
Ammonia
Freon
Brine
Doubling the absolute temperature as well as pressure of the gas
Reducing pressure to one fourth at constant temperature
Reducing temperature to one fourth at constant pressure
Reducing the temperature to half and doubling the pressure
Does not depend upon temperature
Is independent of pressure only
Is independent of volume only
Is independent of both pressure and volume
Heat absorbed
Work done
Both (A) & (B)
Neither (A) nor (B)
d ln p/dt = Hvap/RT2
d ln p/dt = RT2/Hvap
dp/dt = RT2/Hvap
dp/dt = Hvap/RT2
Gibbs-Duhem
Van Laar
Gibbs-Helmholtz
Margules
Pressure
Temperature
Both (A) & (B)
Neither (A) nor (B)
Representing actual behaviour of real gases
Representing actual behaviour of ideal gases
The study of chemical equilibria involving gases at atmospheric pressure
None of these
0°C
273°C
100°C
-273°C
Minimum
Zero
Maximum
None of these
Adiabatic
Isometric
Isentropic
Isothermal
Saturated vapour
Solid
Gas
Liquid
Not liquify (barring exceptions)
Immediately liquify
Never liquify however high the pressure may be
None of these
Increases with rise in pressure
Decreases with rise in pressure
Is independent of pressure
Is a path function