Free energy
Entropy
Refractive index
None of these
C. Refractive index
0
1
2
3
0°C and 750 mm Hg
15°C and 750 mm Hg
0°C and 1 kgf/cm2
15°C and 1 kgf/cm2
Expansion in an engine
Following a constant pressure cycle
Throttling
None of these
Unity
Activity
Both (A) & (B)
Neither (A) nor (B)
Reaction mechanism
Calculation of rates
Energy transformation from one form to another
None of these
Concentration
Mass
Temperature
Entropy
0
1
2
3
Volume of the liquid phase is negligible compared to that of vapour phase
Vapour phase behaves as an ideal gas
Heat of vaporisation is independent of temperature
All (A), (B) & (C)
Triple point
Boiling point
Below triple point
Always
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
Same
Doubled
Halved
One fourth of its original value
Independent of pressure
Independent of temperature
Zero at absolute zero temperature for a perfect crystalline substance
All (A), (B) & (C)
Volume
Density
Temperature
Pressure
λb/Tb
Tb/λb
√(λb/Tb)
√(Tb/λb)
More stable
Less stable
Not at all stable (like nascent O2)
Either more or less stable; depends on the compound
System (of partially miscible liquid pairs), in which the mutual solubility increases with rise in temperature, are said to possess an upper consolute temperature
Systems, in which the mutual solubility increases with decrease in temperature, are said to possess lower consolute temperature
Nicotine-water system shows both an upper as well as a lower consolute temperature, implying that they are partially miscible between these two limiting temperatures
None of these
Cp of monatomic gases such as metallic vapor is about 5 kcal/kg.atom
The heat capacity of solid inorganic substance is exactly equal to the heat capacity of the substance in the molten state
There is an increase in entropy, when a spontaneous change occurs in an isolated system
At absolute zero temperature, the heat capacity for many pure crystalline substances is zero
Minimum
Zero
Maximum
None of these
5 & 3
3.987 & 1.987
1.987 & 0.66
0.66 & 1.987
Volume, mass and number of moles
Free energy, entropy and enthalpy
Both (A) and (B)
None of these
Solution
Formation
Dilution
Combustion
Solids
Liquids
Gases
All (A), (B) & (C)
35 K
174 K
274 K
154 K
Lewis-Randall rule
Statement of Van't Hoff Equation
Le-Chatelier's principle
None of these
Internal energy
Enthalpy
Gibbs free energy
Helmholtz free energy
The net change in entropy in any reversible cycle is always zero
The entropy of the system as a whole in an irreversible process increases
The entropy of the universe tends to a maximum
The entropy of a substance does not remain constant during a reversible adiabatic change
Isobaric
Isothermal
Isentropic
Isometric
Pressure
Temperature
Both (A) & (B)
Neither (A) nor (B)
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
A heating effect
No change in temperature
A cooling effect
Either (A) or (C)