Consider the following reaction:

Question

CO(g) + 2H2(g) - CH4O (g)

Part: 0 / 5

K=2.3×104

Part 1 of 5

Write the expression for the equilibrium constant for this reaction.
Would you predict AH to be positive or negative? Select the single best answer.

zero

positive

negative

Answer 1

The expression for the equilibrium constant for this reaction would be K = [CH4O]/[CO][H2]^2.

Based on Le Chatelier's Principle, if the equilibrium constant K is relatively large, it means that the products are favored at equilibrium. This would suggest that the forward reaction is favored, indicating that the enthalpy change (∆H) is negative. Therefore, the most appropriate answer is negative.