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
D. The fugacity co-efficient is zero for an ideal gas
Isochoric
Isobaric
Adiabatic
Isothermal
Zero
Positive
Negative
None of these
A homogeneous solution (say of phenol water) is formed
Mutual solubility of the two liquids shows a decreasing trend
Two liquids are completely separated into two layers
None of these
Momentum
Mass
Energy
None of these
Vapor pressure
Specific Gibbs free energy
Specific entropy
All (A), (B) and (C)
State functions
Path functions
Intensive properties
Extensive properties
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
Adiabatic expansion
Joule-Thomson effect
Both (A) and (B)
Neither (A) nor (B)
Increases
Decreases
Remains unchanged
May increase or decrease; depends on the gas
The available energy in an isolated system for all irreversible (real) processes decreases
The efficiency of a Carnot engine increases, if the sink temperature is decreased
The reversible work for compression in non-flow process under isothermal condition is the change in Helmholtz free energy
All (A), (B) and (C)
Increase
Decrease
Not alter
None of these
Not a function of its pressure
Not a function of its nature
Not a function of its temperature
Unity, if it follows PV = nRT
(T2 - T1)/T2
(T2 - T1)/T1
(T1 - T2)/T2
(T1 - T2)/T1
Zero
One
Two
Three
0°C and 750 mm Hg
15°C and 750 mm Hg
0°C and 1 kgf/cm2
15°C and 1 kgf/cm2
Number of intermediate chemical reactions involved
Pressure and temperature
State of combination and aggregation in the beginning and at the end of the reaction
None of these
Enthalpy
Volume
Both 'a' & 'b'
Neither 'a' nor 'b'
Steam to ethylene ratio
Temperature
Pressure
None of these
Infinity
Unity
Constant
Negative
P + F - C = 2
C = P - F + 2
F = C - P - 2
P = F - C - 2
The energy change of a system undergoing any reversible process is zero
It is not possible to transfer heat from a lower temperature to a higher temperature
The total energy of system and surrounding remains the same
None of the above
Value of absolute entropy
Energy transfer
Direction of energy transfer
None of these
H = E - PV
H = F - TS
H - E = PV
None of these
2
0
3
1
Ideal
Very high pressure
Very low temperature
All of the above
Binary solutions
Ternary solutions
Azeotropic mixture only
None of these
CO2
H2
O2
N2
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
Extensive property
Intensive property
Force which drives the chemical system to equilibrium
Both (B) and (C)
Bucket
Throttling
Separating
A combination of separating & throttling