Question

The chemical equation below represents a reaction at equilibrium in a closed flask:

CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g) + heat

Which action will cause the reaction to shift to the left?

A) Increasing the temperature
B) Decreasing the pressure
C) Adding more CO
D) Removing some CH4

Answer 1

Increasing the temperature option a, of the equilibrium reaction CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g) will shift the reaction to the left, favoring the reactants.

Step-by-step explanation:

The chemical equation CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g) + heat represents a reaction at equilibrium in a closed flask. The action that will cause the reaction to shift to the left, according to Le Chatelier's principle, is increasing the temperature. This is because the reaction is exothermic (releases heat), and increasing the temperature will favor the endothermic reaction (absorbing heat), which is the reverse process. Option a.