In an exothermic reaction at equilibrium, what effect does decreasing the volume of the reaction container have on the gas mixture ?

Answer and explanation

Correct answer: D. It shifts the equilibrium toward reactants (left)

  1. Step 1: Decreasing container volume increases the total gas pressure.
  2. Step 2: By Le Chatelier's principle, the system shifts toward the side with fewer moles of gas. The left side has 1 mole of gas, while the right side has 2 moles (), so equilibrium shifts left toward .
Answer
It shifts the equilibrium toward reactants (left).
Why not the others: 'Shifts right' occurs if volume is expanded; 'Decreases pressure' is opposite to Boyle's law; 'Zero effect' applies only when moles of gaseous reactants equal products.

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