Which outcome occurs when increased pressure is applied to an equilibrium reaction?

A)Favors side with fewer gas moles✓

B)Equilibrium constant increases exponentially

C)Reaction rate equally favors all sides

D)Activation energy increases drastically

💡 Explanation

Applying Le Chatelier's principle causes a shift in equilibrium, favoring the side with fewer gas moles due to attempting to relieve the applied stress; therefore, the reaction will proceed to consume gas molecules, rather than increase the equilibrium constant or equally affecting all sides.

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Which outcome occurs when increased pressure is applied to an equilibrium reaction?

💡 Explanation

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