Sublimation
Fusion
Transition
Vaporisation
C. Transition
Entropy
Temperature
Enthalpy
Pressure
Isobaric
Adiabatic
Isenthalpic
Both (B) & (C)
V/T = Constant
V ∝ 1/T
V ∝ 1/P
PV/T = Constant
Virial co-efficients are universal constants
Virial co-efficients 'B' represents three body interactions
Virial co-efficients are function of temperature only
For some gases, Virial equations and ideal gas equations are the same
0
+ve
-ve
∞
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
5 & 3
3.987 & 1.987
1.987 & 0.66
0.66 & 1.987
Pressure
Temperature
Both (A) & (B)
Neither (A) nor (B)
Contracts
Expands
Does not change in volume
Either (A), (B) or (C)
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
Decrease in temperature
Increase in temperature
No change in temperature
Change in temperature which is a function of composition
Both the processes are adiabatic
Both the processes are isothermal
Process A is isothermal while B is adiabatic
Process A is adiabatic while B is isothermal
States that n1dμ1 + n2dμ2 + ....njdμj = 0, for a system of definite composition at constant temperature and pressure
Applies only to binary systems
Finds no application in gas-liquid equilibria involved in distillation
None of these
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)
Not a function of its pressure
Not a function of its nature
Not a function of its temperature
Unity, if it follows PV = nRT
Isothermal compression
Isothermal expansion
Adiabatic expansion
Adiabatic compression
Any
A perfect
An easily liquefiable
A real
Molten sodium
Molten lead
Mercury
Molten potassium
Reversible isothermal volume change
Heating of a substance
Cooling of a substance
Simultaneous heating and expansion of an ideal gas
Low temperature
High pressure
Both (A) and (B)
Neither (A) nor (B)
Water
Ammonia
Freon
Brine
Not changed
Decreasing
Increasing
Data sufficient, can't be predicted
0
∞
+ve
-ve
Pressure
Temperature
Both (A) & (B)
Neither (A) nor (B)
Free expansion of a gas
Compression of air in a compressor
Expansion of steam in a turbine
All (A), (B) & (C)
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
R loge 4
R log10 4
Cv log10 4
Cv loge 4
Isothermal
Adiabatic
Isentropic
None of these
Adiabatic expansion
Joule-Thomson effect
Both (A) and (B)
Neither (A) nor (B)
Decreases
Increases
Remain same
May increase or decrease; depends on the nature of the gas