Question

Consider this reaction: Fe₂O₃(s) + 3H₂(g) = 2Fe(s) + 3H₂O(g) ∆H = 98.7 kJ. If this system was in a closed container at equilibrium, and a small amount of hydrogen gas was injected into the container, how would the reaction respond?

a) Making more reactants
b) Making more products
c) Both A and B
d) Noe of the above

Answer 1

Adding hydrogen gas to the reaction at equilibrium will prompt the system to shift towards producing more iron and water vapor to re-establish equilibrium.

Step-by-step explanation:

If a small amount of hydrogen gas (H₂) is added to a closed container at equilibrium containing the reaction Fe₂O₃(s) + 3H₂(g) = 2Fe(s) + 3H₂O(g), according to Le Chatelier's principle, the reaction will respond by making more products to re-establish equilibrium.

This is because the addition of hydrogen increases the concentration of one of the reactants, which drives the reaction towards the formation of more iron (Fe) and water vapor (H₂O(g)).

Additionally, we can see this as a shift in the reaction to the right, towards the products side, in response to the added reactant. The system adjusts by using up excess hydrogen to produce additional iron and water vapor.