Bertholet equation
Clausius-Clapeyron equation
Beattie-Bridgeman equation
None of these
B. Clausius-Clapeyron equation
Equal to its density
The reciprocal of its density
Proportional to pressure
None of these
Single phase fluid of varying composition
Single phase fluid of constant composition
Open as well as closed systems
Both (B) and (C)
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
(R/ΔH) (1/T1 - 1/T2)
(ΔH/R) (1/T1 - 1/T2)
(ΔH/R) (1/T2 - 1/T1)
(1/R) (1/T1 - 1/T2)
Isolated
Closed
Open
None of these
Pressure
Temperature
Both (A) & (B)
Neither (A) nor (B)
Zero
Unity
Infinity
An indeterminate value
Below
At
Above
Either 'b' or 'c'
Increases
Decreases
Remains unchanged
May increase or decrease; depends on the substance
Internal energy
Enthalpy
Entropy
All (A), (B) & (C)
Zero
Negative
Very large compared to that for endothermic reaction
Not possible to predict
Gibbs-Duhem
Van Laar
Gibbs-Helmholtz
Margules
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
d ln p/dt = Hvap/RT2
d ln p/dt = RT2/Hvap
dp/dt = RT2/Hvap
dp/dt = Hvap/RT2
Expansion of a real gas
Reversible isothermal volume change
Heating of an ideal gas
Cooling of a real gas
Always exists
May exist
Never exists
Is difficult to predict
Simultaneous pressure & temperature change
Heating
Cooling
Both (B) and (C)
0
1
2
3
Low pressure and high temperature
Low pressure and low temperature
Low temperature and high pressure
High temperature and high pressure
Entropy
Internal energy
Enthalpy
Gibbs free energy
A real gas on expansion in vacuum gets heated up
An ideal gas on expansion in vacuum gets cooled
An ideal gas on expansion in vacuum gets heated up
A real gas on expansion in vacuum cools down whereas ideal gas remains unaffected
Zero
One
Infinity
Negative
Δ H = 0 and ΔS = 0
Δ H ≠ 0 and ΔS = 0
Δ H ≠ 0 and ΔS ≠ 0
Δ H = 0 and ΔS ≠ 0
Carnot
Air
Absorption
vapour-ejection
Zero
Unity
Infinity
None of these
Two different gases behave similarly, if their reduced properties (i.e. P, V and T) are same
The surface of separation (i. e. the meniscus) between liquid and vapour phase disappears at the critical temperature
No gas can be liquefied above the critical temperature, howsoever high the pressure may be.
The molar heat of energy of gas at constant volume should be nearly constant (about 3 calories)
With pressure changes at constant temperature
Under reversible isothermal volume change
During heating of an ideal gas
During cooling of an ideal gas
Increases
Decreases
Remains unchanged
Data insufficient, can't be predicted
More
Less
Same
Data insufficient to predict
Increase
Decrease
Remain unaltered
Increase or decrease; depends on the particular reaction