Always exists
May exist
Never exists
Is difficult to predict
The amount of work needed is path dependent
Work alone cannot bring out such a change of state
The amount of work needed is independent of path
More information is needed to conclude anything about the path dependence or otherwise of the work needed
Minimum number of degree of freedom of a system is zero
Degree of freedom of a system containing a gaseous mixture of helium, carbon dioxide and hydrogen is 4
For a two phase system in equilibrium made up of four non-reacting chemical species, the number of degrees of freedom is 4
Enthalpy and internal energy change is zero during phase change processes like melting, vaporisation and sublimation
Mass
Energy
Momentum
None of these
P ∝ 1/V, when temperature is constant
P ∝ 1/V, when temperature & mass of the gas remain constant
P ∝ V, at constant temperature & mass of the gas
P/V = constant, for any gas
Internal energy
Enthalpy
Gibbs free energy
Helmholtz free energy
T1/(T1-T2)
T2/(T1-T2)
T1/T2
T2/R1
Polar
Non-polar
Both (A) & (B)
Neither (A) nor (B)
Concentration of the constituents only
Quantities of the constituents only
Temperature only
All (A), (B) and (C)
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
R loge 4
R log10 4
Cv log10 4
Cv loge 4
P + F - C = 2
C = P - F + 2
F = C - P - 2
P = F - C - 2
Gibbs-Duhem equation
Gibbs-Helmholtz equation
Third law of thermodynamics
Joule-Thomson effect
Zero
+ve
-ve
Dependent on the path
Two
One
Zero
Three
Critical properties
Specific gravity
Specific volume
Thermal conductivity
5 & 3
3.987 & 1.987
1.987 & 0.66
0.66 & 1.987
270
327
300
540
Same in both the phases
Zero in both the phases
More in vapour phase
More in liquid phase
V1/V2
V2/V1
V1 - V2
V1.V2
Increases
Decreases
Remain same
Decreases linearly
Melting of ice
Condensation of alcohol vapor
Sudden bursting of a cycle tube
Evaporation of water
λb/Tb
Tb/λb
√(λb/Tb)
√(Tb/λb)
Low temperature
High pressure
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)
Molecular size
Volume
Pressure
Temperature
State function
Macroscopic property
Extensive property
None of these
Reversible and isothermal
Irreversible and constant enthalpy
Reversible and constant entropy
Reversible and constant enthalpy
x
x + 1
x + 2
x + 3
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