Question

2h₂o₂ ⇌ 2h₂o + o₂ if more o₂ is added, which direction will the equilibrium shift to reestablish the balance? hint: the shift should use up what is added. the equilibrium will shift randomly without a predictable direction. the equilibrium will shift to the left, forming more h₂o₂. the equilibrium will remain unchanged. the equilibrium will shift to the right, forming more h₂o and o₂.

Explanation:

To solve this, we use Le Chatelier's Principle, which states that if a stress (like adding a product) is applied to a system at equilibrium, the system will shift to counteract that stress. Here, \( \ce{O2} \) is a product (on the right side of the equilibrium \( \ce{2H2O2
ightleftharpoons 2H2O + O2} \)). Adding more \( \ce{O2} \) (a product) will cause the equilibrium to shift left (towards the reactants, \( \ce{H2O2} \)) to use up the excess \( \ce{O2} \).

• The first option is wrong because equilibrium shifts are predictable via Le Chatelier's Principle.
• The third option is wrong because adding a product will disturb the equilibrium, so it can't remain unchanged.
• The fourth option is wrong because shifting right would produce more \( \ce{O2} \), which is already in excess, worsening the stress.
• The second option is correct: shifting left uses up \( \ce{O2} \) by converting it back to \( \ce{H2O2} \).

Answer:

The equilibrium will shift to the left, forming more \( \ce{H2O2} \).