Freezing
Triple
Boiling
Boyle
B. Triple
Isometric
Polytropic
Isentropic
Isobaric
Bomb
Separating
Bucket
Throttling
Equilibrium cannot be established
More ice will be formed
More water will be formed
Evaporation of water will take place
The melting point of wax
The boiling point of a liquid
Both (A) and (B)
Neither (A) nor (B)
A gas may have more than one inversion temperatures
The inversion temperature is different for different gases
The inversion temperature is same for all gases
The inversion temperature is the temperature at which Joule-Thomson co-efficient is infinity
Lewis-Randall
Margules
Van Laar
Both (B) & (C)
RT ln K
-RT ln K
-R ln K
T ln K
Kp2/Kp1 = - (ΔH/R) (1/T2 - 1/T1)
Kp2/Kp1 = (ΔH/R) (1/T2 - 1/T1)
Kp2/Kp1 = ΔH (1/T2 - 1/T1)
Kp2/Kp1 = - (1/R) (1/T2 - 1/T1)
No
Any real
Only ideal
Both (B) and (C)
Superheated
Desuperheated
Non-condensable
None of these
Tds = dE - dW = 0
dE - dW - Tds = 0
Tds - dE + dW < 0
Tds - dT + dW < 0
∞
0
< 0
> 0
Isobaric
Isothermal
Adiabatic
None of these
Less pronounced
More pronounced
Equal
Data insufficient, can't be predicted
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)
Superheated vapour
Partially condensed vapour with quality of 0.9
Saturated vapour
Partially condensed vapour with quality of 0.1
0
1
∞
None of these
At low temperature and high pressure
At standard state
Both (A) and (B)
In ideal state
+ve
-ve
0
Either of the above three; depends on the nature of refrigerant
TR/(T2 - TR) × (T1 - T2)/T1
TR/(T2 - TR) × T1/(T1 - T2)
TR/(T1 - TR) × (T1 - T2)/T1
None of these
Zero
Positive
Negative
None of these
It is exothermic
It is isenthalpic
It takes place isothermally
It takes place at constant volume
Less
More
Same
Dependent on climatic conditions
In an isothermal system, irreversible work is more than reversible work
Under reversible conditions, the adiabatic work is less than isothermal work
Heat, work, enthalpy and entropy are all 'state functions'
Matter and energy cannot be exchanged with the surroundings in a closed system
Two isothermal and two isentropic
Two isobaric and two isothermal
Two isochoric and two isobaric
Two isothermals and two isochoric
The surface tension vanishes
Liquid and vapour have the same density
There is no distinction between liquid and vapour phases
All (A), (B) and (C)
Entropy
Gibbs energy
Internal energy
Enthalpy
Unity
Activity
Both (A) & (B)
Neither (A) nor (B)
Enthalpy remains constant
Entropy remains constant
Temperature remains constant
None of these
Activity co-efficient is dimensionless.
In case of an ideal gas, the fugacity is equal to its pressure.
In a mixture of ideal gases, the fugacity of a component is equal to the partial pressure of the component.
The fugacity co-efficient is zero for an ideal gas