Consider the following reaction:
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
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.