Question

Consider this reaction: Fe₂O₃(s) + 3H₂(g) = 2Fe(s) + 3H₂O(g). If hydrogen gas is injected into the closed container at equilibrium, how would the reaction shift?

a) Making more reactants
b) Making more products
c) No change in the equilibrium
d) A shift in both reactants and products

Answer 1

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

Step-by-step explanation:

If hydrogen gas is injected into the closed container at equilibrium, the reaction would shift towards making more products. This is because the added hydrogen will increase the concentration of the reactant, causing the equilibrium to shift in the forward direction to reduce the added hydrogen. As a result, more products, which are Fe(s) and H2O(g), will be formed.