Isolated
Closed
Open
None of these
C. Open
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
Isolated
Closed
Open
None of these
Steam to ethylene ratio
Temperature
Pressure
None of these
Critical temperature
Melting point
Freezing point
Both (B) and (C)
Increases
Decreases
Remains unchanged
May increase or decrease; depends on the substance
T2/(T1 - T2)
T1/(T1 - T2)
(T1 - T2)/T1
(T1 - T2)/T2
Increase
Decrease
Remain unaltered
Increase or decrease; depends on the particular reaction
Zero
Positive
Negative
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
Reaction mechanism
Calculation of rates
Energy transformation from one form to another
None of these
Adiabatic process
Endothermic reaction
Exothermic reaction
Process involving a chemical reaction
Water
Ammonia
Freon
Brine
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
CV
Entropy change
Gibbs free energy
None of these
Cold reservoir approaches zero
Hot reservoir approaches infinity
Either (A) or (B)
Neither (A) nor (B)
Slower than Y
Faster than Y
Three times slower than Y
Three times faster than Y
The expansion of a gas in vacuum is an irreversible process
An isometric process is a constant pressure process
Entropy change for a reversible adiabatic process is zero
Free energy change for a spontaneous process is negative
V/T = Constant
V ∝ 1/T
V ∝ 1/P
PV/T = Constant
12 P1V1
6 P1 V1
3 P1V1
P1 V1
Same
Doubled
Halved
One fourth of its original value
Shift the equilibrium towards right
Give higher yield of NH3
Both (B) and (C)
Neither (A) nor (B)
Infinity
Unity
Constant
Negative
Entropy
Gibbs free energy
Internal energy
All (A), (B) & (C)
Process must be isobaric
Temperature must decrease
Process must be adiabatic
Both (B) and (C)
Free energy
Entropy
Refractive index
None of these
Vapor pressure
Partial pressure
Chemical potential
None of these
Escaping tendencies of the same substance in different phases of a system
Relative volatility of a mixture of two miscible liquids
Behaviour of ideal gases
None of these
Isothermal
Isentropic
Isobaric
Adiabatic
0
∞
50
100
Pressure to critical pressure
Critical pressure to pressure
Pressure to pseudocritical pressure
Pseudocritical pressure to pressure