Which one of the following statements is true about the equilibrium constant for a reaction if δg° for the reaction is negative? k > 1 k < 1 k = 1 k = 0

Answer : K > 1is the true statement about the equilibrium constant for a reaction if for the reaction is negative.

Explanation :

The relation between the equilibrium constant and standard Gibbs, free energy is:

where,

= standard Gibbs, free energy

R = gas constant

T = temperature

K = equilibrium constant

From the above relation we conclude that,

When K > 1 then the value of is negative.

When K < 1 then the value of is positive.

When K = 1 then the value of is zero.

When K = 0 then the value of is undefined.

Hence, K > 1is the true statement about the equilibrium constant for a reaction if for the reaction is negative.

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