Question

The equilibrium constant describes a ratio between the concentrations of the products and the reactants. If...

The equilibrium constant describes a ratio between the concentrations of the products and the reactants. If the free energy of this equilibrium is -0.212kJ mol-1 K-1 for room temperature, what temperature will be required to force the equilibrium to greater than 95% in favor of the products?

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Answer #1

Ans Delta G = - R T lnKeq

= -2.303 * 8.314 * 298 log Keq

-0.212* 1000 = - 5705.8 logKeq

logKeq = 0.037

Keq = 1.088

At room temperature, ratio of the concentration of product to the concentration of the reactants is almost equal.

For 95 % in favour of the product, Keq = 1.088 * 1.95 = 2.12

delta G = - 2.303 * 8.314 * T log(2.12)

T = 212/ 6.241 = 33.96K

That indicates the forward reaction is exothermic and on lowering the temperature to 33.96K, the equilibrium will be greater than 95% in favor of the products.

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