Question

If the equation for equilibrium constant represents products over reacants that are raised to their coefficients, which is the correct balanced chemical equation that would yield a K = 8.0 when the values of everything at equilibrium are [CO] = 1.5, [H_2] = 2.0, [CH_4] = 2.0, and [H_2O] = 4.0?

(A) CO + 2H_2 <=> CH_4 + H_2O
(B) CO + 3H_2 <=> CH_4 + 2H_2O
(C) CO + 4H_2 <=> CH_4 + 3H_2O
(D) CO + 5H_2 <=> CH_4 + 4H_2O

Answer 1

The correct balanced chemical equation that would yield a K = 8.0 when the values at equilibrium are given is CO + 4H₂ <=> CH₄ + 3H₂O.

Step-by-step explanation:

The correct balanced chemical equation that would yield a K = 8.0 when the values of everything at equilibrium are [CO] = 1.5, [H₂] = 2.0, [CH₄] = 2.0, and [H₂O] = 4.0 is option (C): CO + 4H₂ <=> CH₄ + 3H₂O.

To find the correct equation, we need to use the given values of the concentrations at equilibrium and the equation for the equilibrium constant (K). We can plug the given values into the equation, [CH₄][H₂O]³ / [CO][H₂]⁴, and solve for K. Option (C) is the only equation that, when plugged into the K equation, yields a K value of 8.0.

Therefore, the correct balanced chemical equation that would yield a K = 8.0 is CO + 4H₂ <=> CH₄ + 3H₂O.