+ve
0
-ve
∞
A. +ve
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
Surface tension
Free energy
Specific heat
Refractive index
First law
Zeroth law
Third law
Second law
Increase
Decrease
Remain unchanged
First fall and then rise
Reversible isothermal
Irreversible isothermal
Reversible adiabatic
None of these
High temperature
Low pressure
Low temperature only
Both low temperature and high pressure
Endothermic
Exothermic
Isothermal
Adiabatic
30554
10373
4988.4
4364.9
Is increasing
Is decreasing
Remain constant
Data insufficient, can't be predicted
Polar
Non-polar
Both (A) & (B)
Neither (A) nor (B)
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)
Heat pump
Heat engine
Carnot engine
None of these
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
Steam to ethylene ratio
Temperature
Pressure
None of these
If an insoluble gas is passed through a volatile liquid placed in a perfectly insulated container, the temperature of the liquid will increase
A process is irreversible as long as Δ S for the system is greater than zero
The mechanical work done by a system is always equal to∫P.dV
The heat of formation of a compound is defined as the heat of reaction leading to the formation of the compound from its reactants
Addition of inert gas favours the forward reaction, when Δx is positive
Pressure has no effect on equilibrium, when Δn = 0
Addition of inert gas has no effect on the equilibrium constant at constant volume for any value of Δx (+ ve, - ve) or zero)
All 'a', 'b' & 'c'
V1/V2
V2/V1
V1 - V2
V1.V2
H = E - PV
H = F - TS
H - E = PV
None of these
Enthalpy
Pressure
Entropy
None of these
Less pronounced
More pronounced
Equal
Data insufficient, can't be predicted
Infinity
Minus infinity
Zero
None of these
0
273
25
None of these
Pressure remains constant
Pressure is increased
Temperature remains constant
None of these
A heating effect
No change in temperature
A cooling effect
Either (A) or (C)
Expansion of an ideal gas against constant pressure
Atmospheric pressure vaporisation of water at 100°C
Solution of NaCl in water at 50°C
None of these
Increase the partial pressure of I2
Decrease the partial pressure of HI
Diminish the degree of dissociation of HI
None of these
(dF)T, p < 0
(dF)T, p > 0
(dF)T, p = 0
(dA)T, v < 0
The amount of work needed is path dependent
Work alone cannot bring out such a change of state
The amount of work needed is independent of path
More information is needed to conclude anything about the path dependence or otherwise of the work needed
Solution
Formation
Dilution
Combustion
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)