Question

Consider the chemical equation in equilibrium. CH4(g) + H2O(g) mc029-1.jpg CO(g) + 3H2(g) What will happen to the equilibrium of this reaction if the pressure is increased? The equilibrium will shift to the left to favor the reverse reaction. The equilibrium will shift to the right to favor the forward reaction. The equilibrium will not be affected by changing the pressure. The equilibrium will not be reestablished after this kind of stress.

Answer 1

Answer:

A. The equilibrium will shift to the left to favor the reverse reaction

Explanation:

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Answer 2

Answer: The equilibrium will shift to the left to favor the reverse reaction.

Explanation:

This is a direct application of Le Chatelier's principle.

Le Chatelier's principle predicts that if a chage is introduced in a system in equilibrium, the system will react to compensate the change.

The increase in the concentration of CO, which is in the right side of the chemical equation,  takes the system out of the equilibrium.

Chemically, the greater number of molecules of CO means that more CO will react to favor the reverse reaction and restore the equilibrium with the increase of molecules in the left side (CH4 and H2O).