Less
More
Same
More or less depending upon the extent of work done
B. More
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
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)
(R/ΔH) (1/T1 - 1/T2)
(ΔH/R) (1/T1 - 1/T2)
(ΔH/R) (1/T2 - 1/T1)
(1/R) (1/T1 - 1/T2)
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
Isolated
Open
Insulated
Closed
Van Laar
Margules
Gibbs-Duhem
Gibbs-Duhem-Margules
dE = CpdT
dE = CvdT
dQ = dE + pdV
dW = pdV
Increases, for an exothermic reaction
Decreases, for an exothermic reaction
Increases, for an endothermic reaction
None of these
Temperature
Specific heat
Volume
Pressure
Tds = dE - dW = 0
dE - dW - Tds = 0
Tds - dE + dW < 0
Tds - dT + dW < 0
A heating effect
No change in temperature
A cooling effect
Either (A) or (C)
Increases
Decreases
Remain same
Decreases linearly
Increases
Decreases
Remain constant
Increases linearly
Specific volume
Temperature
Mass
Pressure
Only ΔE = 0
Only ΔH =0
ΔE = ΔH = 0
dQ = dE
Heat capacity of a crystalline solid is zero at absolute zero temperature
Heat transfer from low temperature to high temperature source is not possible without external work
Gases having same reduced properties behaves similarly
None of these
Temperature
Pressure
Volume
Entropy
Not changed
Decreasing
Increasing
Data sufficient, can't be predicted
Decrease on addition of Cl2
Increase on addition of an inert gas at constant pressure
Decrease on increasing the pressure of the system
None of these
Pressure
Temperature
Volume
Molar concentration
Entropy
Gibbs free energy
Internal energy
All (A), (B) & (C)
Negative
Zero
Infinity
None of these
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'
Phase rule variables are intensive properties
Heat and work are both state function
The work done by expansion of a gas in vacuum is zero
CP and CV are state function
270
327
300
540
Reversible
Irreversible
Isothermal
Adiabatic
At constant pressure
By throttling
By expansion in an engine
None of these
Solution
Formation
Dilution
Combustion
Δ H = 0 and ΔS = 0
Δ H ≠ 0 and ΔS = 0
Δ H ≠ 0 and ΔS ≠ 0
Δ H = 0 and ΔS ≠ 0
Expansion in an engine
Following a constant pressure cycle
Throttling
None of these