Vapor pressure
Partial pressure
Chemical potential
None of these
B. Partial pressure
At constant pressure, solubility of a gas in a liquid diminishes with rise in temperature
Normally, the gases which are easily liquefied are more soluble in common solvents
The gases which are capable of forming ions in aqueous solution are much more soluble in water than in other solvents
At constant pressure, solubility of a gas in a liquid increases with rise in temperature
d ln p/dt = Hvap/RT2
d ln p/dt = RT2/Hvap
dp/dt = RT2/Hvap
dp/dt = Hvap/RT2
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
ds = 0
ds < 0
ds > 0
ds = Constant
Decreases in all spontaneous (or irreversible) processes
Change during a spontaneous process has a negative value
Remains unchanged in reversible processes carried at constant temperature and pressure
All (A), (B) and (C)
-19.4
-30.2
55.2
-55.2
State function
Macroscopic property
Extensive property
None of these
Lewis-Randall
Margules
Van Laar
Both (B) & (C)
The melting point of wax
The boiling point of a liquid
Both (A) and (B)
Neither (A) nor (B)
Always greater than one
Same at the same reduced temperature
Same at the same reduced pressure
Both (B) & (C)
Expansion in an engine
Following a constant pressure cycle
Throttling
None of these
Decrease in velocity
Decrease in temperature
Decrease in kinetic energy
Energy spent in doing work
Water
Ammonia
Freon
Brine
Solid-vapor
Solid-liquid
Liquid-vapor
All (A), (B) and (C)
6738.9
6753.5
7058.3
9000
Increase
Decrease
Not alter
None of these
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
Mole fraction
Fugacity at the same temperature and pressure
Partial pressure
None of these
λb/Tb
Tb/λb
√(λb/Tb)
√(Tb/λb)
1.572
1.9398
3.389
4.238
An ideal liquid or solid solution is defined as one in which each component obeys Raoult's law
If Raoult's law is applied to one component of a binary mixture; Henry's law or Raoult's law is applied to the other component also
Henry's law is rigorously correct in the limit of infinite dilution
None of these
Is zero
Increases
Decreases whereas the entropy increases
And entropy both decrease
(∂E/∂ni)S, v, nj
(∂G/∂ni)T, P, nj = (∂A/∂ni) T, v, nj
(∂H/∂ni)S, P, nj
All (A), (B) and (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
Trouton's ratio of non-polar liquids is calculated using Kistyakowsky equation
Thermal efficiency of a Carnot engine is always less than 1
An equation relating pressure, volume and temperature of a gas is called ideal gas equation
None of these
Isothermal
Irreversible
Adiabatic
Reversible
0°C and 750 mm Hg
15°C and 750 mm Hg
0°C and 1 kgf/cm2
15°C and 1 kgf/cm2
Heat capacity
Molal heat capacity
Pressure
Concentration
Evaporation
Liquid extraction
Drying
Distillation
(∂T/∂V)S = (∂p/∂S)V
(∂T/∂P)S = (∂V/∂S)P
(∂P/∂T)V = (∂S/∂V)T
(∂V/∂T)P = -(∂S/∂P)T