x
x + 1
x + 2
x + 3
C. x + 2
Latent heat of vaporisation
Chemical potential
Molal boiling point
Heat capacity
Temperature
Mass
Volume
Pressure
At constant pressure
By throttling
By expansion in an engine
None of these
100,000 kW
160,000 kW
200,000 kW
320,000 kW
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
Enthalpies of all elements in their standard states are assumed to be zero
Combustion reactions are never endothermic in nature
Heat of reaction at constant volume is equal to the change in internal energy
Clausius-Clapeyron equation is not applicable to melting process
0
1
y = 1.44
1.66
Adiabatic
Isothermal
Isometric
None of these
Mole fraction
Activity
Pressure
Activity co-efficient
Entropy
Gibbs free energy
Internal energy
All (A), (B) & (C)
Use of only one graph for all gases
Covering of wide range
Easier plotting
More accurate plotting
P + F - C = 2
C = P - F + 2
F = C - P - 2
P = F - C - 2
(atm)Δx, when Δx is negative
(atm)Δx, when Δx is positive
Dimensionless, when Δx = 0
(atm)Δx2, when Δx > 0
Independent of pressure
Independent of temperature
Zero at absolute zero temperature for a perfect crystalline substance
All (A), (B) & (C)
ΔF = ΔH + T [∂(ΔF)/∂T]P
ΔF = ΔH - TΔT
d(E - TS) T, V < 0
dP/dT = ΔHvap/T.ΔVvap
Adiabatic process
Isothermal process
Isobaric process
All require same work
Decrease in temperature
Increase in temperature
No change in temperature
Change in temperature which is a function of composition
Phase rule variables are intensive properties
Heat and work are both state function
The work done by expansion of a gas in vacuum is zero
CP and CV are state function
0°C and 760 mm Hg
15°C and 760 mm Hg
20°C and 760 mm Hg
0°C and 1 kgf/cm2
349
651
667
1000
Joule-Thomson co-efficient
Specific heat at constant pressure (Cp)
co-efficient of thermal expansion
Specific heat at constant volume (CV)
Direction of energy transfer
Reversible processes only
Irreversible processes only
None of these
Volume
Pressure
Temperature
All (A), (B) and (C)
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
1.987 cal/gm mole °K
1.987 BTU/lb. mole °R
Both (A) and (B)
Neither (A) nor (B)
0.5
3.5
4.5
8.5
Zero
+ve
-ve
Dependent on the path
RT ln K
-RT ln K
-R ln K
T ln K
Solubility increases as temperature increases
Solubility increases as temperature decreases
Solubility is independent of temperature
Solubility increases or decreases with temperature depending on the Gibbs free energy change of solution
Adiabatic
Isothermal
Isometric
None of these