Same
Doubled
Halved
One fourth of its original value
A. Same
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
< 0
> 0
= 0
None of these
P1ACBP2P1
ACBB1A1A
ACBDA
ADBB1A1A
Isothermal
Adiabatic
Isobaric
Isometric
Gibbs-Duhem
Van Laar
Gibbs-Helmholtz
Margules
Increase
Decrease
Remain unaltered
Increase or decrease; depends on the particular reaction
Increases
Decreases
Remain same
Decreases linearly
dQ = dE + dW
dQ = dE - dW
dE = dQ + dW
dW = dQ + dE
Internal energy
Enthalpy
Gibbs free energy
Helmholtz free energy
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
0°C and 760 mm Hg
15°C and 760 mm Hg
20°C and 760 mm Hg
0°C and 1 kgf/cm2
Decreases
Increases
Remain same
Decreases linearly
(atm)Δx, when Δx is negative
(atm)Δx, when Δx is positive
Dimensionless, when Δx = 0
(atm)Δx2, when Δx > 0
The chemical potential of a pure substance depends upon the temperature and pressure
The chemical potential of a component in a system is directly proportional to the escaping tendency of that component
The chemical potential of ith species (μi) in an ideal gas mixture approaches zero as the pressure or mole fraction (xi) tends to be zero at constant temperature
The chemical potential of species 'i' in the mixture (μi) is mathematically represented as,μi = ∂(nG)/∂ni]T,P,nj where, n, ni and nj respectively denote the total number of moles, moles of ith species and all mole numbers except ith species. 'G' is Gibbs molar free energy
Fugacity
Activity co-efficient
Free energy
All (A), (B) & (C)
Process must be isobaric
Temperature must decrease
Process must be adiabatic
Both (B) and (C)
T
T and P
T, P and Z
T and Z
Entropy
Temperature
Enthalpy
Pressure
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
[∂(G/T)/∂T] = - (H/T2)
[∂(A/T)/∂T]V = - E/T2
Both (A) and (B)
Neither (A) nor (B)
Le-Chatelier principle
Kopp's rule
Law of corresponding state
Arrhenius hypothesis
Enthalpy
Pressure
Entropy
None of these
Less than
Equal to
More than
Either (B) or (C); depends on the type of alloy
The expansion of a gas in vacuum is an irreversible process
An isometric process is a constant pressure process
Entropy change for a reversible adiabatic process is zero
Free energy change for a spontaneous process is negative
0
∞
+ ve
- ve
Increase the partial pressure of I2
Decrease the partial pressure of HI
Diminish the degree of dissociation of HI
None of these
A refrigeration cycle violates the second law of thermodynamics
Refrigeration cycle is normally represented by a temperature vs. entropy plot
In a refrigerator, work required decreases as the temperature of the refrigerator and the temperature at which heat is rejected increases
One ton of refrigeration is equivalent to the rate of heat absorption equal to 3.53 kW
Kinematic viscosity
Work
Temperature
None of these
Entropy
Temperature
Internal energy
Enthalpy
Zeroth
First
Second
Third