Question

Consider the following reaction at equilibrium:

Fe₂O₃(s)+3H₂(g)⇌2Fe(s)+3H₂O(G) ΔH=98.7kJ

If a small amount of hydrogen gas is injected into the closed container at equilibrium, which direction would the reaction shift towards?

Options:
1) Producing more reactants
2) Producing more products

Answer 1

If hydrogen gas is injected into the closed container at equilibrium, the reaction will shift towards producing more products.

Step-by-step explanation:

At equilibrium, the reaction Fe₂O₃(s) + 3H₂(g) ⇌ 2Fe(s) + 3H₂O(g) is balanced, meaning the rate of the forward and reverse reactions are equal. If a small amount of hydrogen gas is injected into the closed container at equilibrium, the reaction will shift towards the production of more products, 2Fe(s) + 3H₂O(g). This is because the addition of more reactant (H₂) will cause the equilibrium to shift in the direction that consumes the added reactant, resulting in an increase in product concentration.