Question

Which of the following two reactions would have an equilibrium constant more favorable to the right? Explain your answer.

Answer 1

(1) Q < K    or   K > 1 reactions quilibrium constant more favorable to the right.

(2) Q > K   or K < 1 reactions quilibrium constant more favorable to the left

(3) Q = K or K = 1 , no shift . exactly at equilibrium

example:

suppose equilibrium concentrations of [H2] = 1 , [I2] = 2 M , [HI] = 3 M. the equilibrium shifts in which direction?

H2 + I2 <-------------------> 2HI

1       2                               3

K = [HI]^2 /[H2][I2]

K = 3^2 / 1 x 2

K = 4.5

here K > 1 so the reaction shifts to the right i.e product side.

note : i did not see any reactions in your question . so i am explaining in this way.

if you need any doubt upload your reactions . iam ready to solve.