Chemical Engineering Thermodynamics
In a reversible chemical reaction (where, Δx = number of moles of products-number of moles of reactants )

Pressure has no effect on equilibrium, when Δn = 0
Addition of inert gas favours the forward reaction, when Δx is positive
All of these
Addition of inert gas has no effect on the equilibrium constant at constant volume for any value of Δx (+ ve, - ve) or zero)

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Chemical Engineering Thermodynamics
On a P-V diagram of an ideal gas, suppose a reversible adiabatic line intersects a reversible isothermal line at point A. Then at a point A, the slope of the reversible adiabatic line (∂P/∂V)S and the slope of the reversible isothermal line (∂P/∂V)T are related as (where, y = Cp/Cv) )

(∂P/∂V)S = 1/y(∂P/∂V)T
(∂P/∂V)S = [(∂P/∂V)T]Y
(∂P/∂V)S = (∂P/∂V)T
(∂P/∂V)S = y(∂P/∂V)T

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