For N₂(g) + 3H₂(g) ⇌ 2NH₃(g), what is the effect of increasing the total pressure at constant temperature?
Correct answer B. The equilibrium shifts to the right because fewer gas molecules are on that side
Explanation
Four moles of gas react to give two moles. By Le Chatelier's principle, higher pressure favours the side with fewer gas molecules, so more NH₃ forms. Kc itself changes only with temperature.
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