Question

Given the reaction: H2O2(l) ⇌ H2(g) + O2(g) The forward reaction is endothermic. Determine which of the following changes would result in equilibrium shifting towards the reactants.

I. Increase H2
II. Decrease O2
III. Add a catalyst
IV. Decrease the temperature
V. Increase H2O2

Answer 1

Answer: all I know it’s not I and II

Step-by-step explanation:

Answer 2

I and IV

Step-by-step explanation:

Increasing the number of particles at one side of the reaction (H2 in this case) results in the shifting of the equilibrium to the side with lesser number of particles, so in this case the equilibrium will shift to the left (towards the reactants)

A decrease in temperature will always function to favor the exothermic reaction, and since the backwards reaction is exothermic, the equilibrium will shift to the left (towards the reactants).

Option II and V will shift the equilibrium to the products, and adding a catalyst has no effect on the equilibrium.

Hope this helps!