Question

3 attempts left Check my work At a given temperature, the equilibrium constant for a certain reaction is 1 x 1026. Does this equilibrium favor products or reactants? Why? Select the single best answer. A large value for the equilibrium constant favors reactant formation. A small value for the equilbrium constant favors product formation. Significant concentrations of both products and reactants are present at equilibrium. A large value for the equilibrium constant favors product formation. A small value for the equilbrium constant favors reactant formation.

Answer 1

Equilibrium constant is ratio of "rate of forward reaction" to "rate of backward reaction"

so

K_{eq = (}rate of forward reaction) / (rate of backward reaction)

so in favor of formation of product K_eq should be large or greater than 1 (one) so that

(Rate)_forward > (Rate)_backward

than 4^{th option is correct}