CO2
H2
O2
N2
B. H2
Increase the partial pressure of H2
Increase the partial pressure of I2
Increase the total pressure and hence shift the equilibrium towards the right
Not affect the equilibrium conditions
Increases with rise in pressure
Decreases with rise in pressure
Is independent of pressure
Is a path function
The distribution law
Followed from Margules equation
A corollary of Henry's law
None of these
Tds = dE - dW = 0
dE - dW - Tds = 0
Tds - dE + dW < 0
Tds - dT + dW < 0
Simultaneous pressure & temperature change
Heating
Cooling
Both (B) and (C)
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
Both the processes are adiabatic
Both the processes are isothermal
Process A is isothermal while B is adiabatic
Process A is adiabatic while B is isothermal
Van Laar
Margules
Gibbs-Duhem
Gibbs-Duhem-Margules
1st
Zeroth
3rd
None of these
Gibbs-Duhem equation
Gibbs-Helmholtz equation
Third law of thermodynamics
Joule-Thomson effect
Bertholet equation
Clausius-Clapeyron equation
Beattie-Bridgeman equation
None of these
0
∞
+ve
-ve
Lewis-Randall rule
Statement of Van't Hoff Equation
Le-Chatelier's principle
None of these
Rate of change of vapour pressure with temperature
Effect of an inert gas on vapour pressure
Calculation of ΔF for spontaneous phase change
Temperature dependence of heat of phase transition
dE = Tds - PdV
dQ = CvdT + PdV
dQ = CpdT + Vdp
Tds = dE - PdV
Isolated
Open
Insulated
Closed
State function
Macroscopic property
Extensive property
None of these
Cp of monatomic gases such as metallic vapor is about 5 kcal/kg.atom
The heat capacity of solid inorganic substance is exactly equal to the heat capacity of the substance in the molten state
There is an increase in entropy, when a spontaneous change occurs in an isolated system
At absolute zero temperature, the heat capacity for many pure crystalline substances is zero
It is exothermic
It is isenthalpic
It takes place isothermally
It takes place at constant volume
Third law of thermodynamics
Second law of thermodynamics
Nernst heat theorem
Maxwell's relations
Prediction of the extent of a chemical reaction
Calculating absolute entropies of substances at different temperature
Evaluating entropy changes of chemical reaction
Both (B) and (C)
1
2
3
4
Pressure and temperature
Reduced pressure and reduced temperature
Critical pressure and critical temperature
None of these
Pressure
Temperature
Both (A) & (B)
Neither (A) nor (B)
Decrease in velocity
Decrease in temperature
Decrease in kinetic energy
Energy spent in doing work
Increases
Decreases
Remains unchanged
Data insufficient, can't be predicted
Molar concentration
Quantity (i.e. number of moles)
Both (A) and (B)
Neither (A) nor (B)
x
x + 1
x + 2
x + 3
Bomb
Separating
Bucket
Throttling
Minimum number of degree of freedom of a system is zero
Degree of freedom of a system containing a gaseous mixture of helium, carbon dioxide and hydrogen is 4
For a two phase system in equilibrium made up of four non-reacting chemical species, the number of degrees of freedom is 4
Enthalpy and internal energy change is zero during phase change processes like melting, vaporisation and sublimation