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

Answer 1

Answer:

Option(II) and option (IV) are correct.

Explanation:

Here products are $H_{2}$ and $O_{2}$ and reactant is $H_{2}O_{2}$

(I) According to Le-chatelier principle,increase in $H_{2}$  will shift the equilibrium towards reactant side to keep the equilibrium constant unchanged.

(II) According to Le-chatelier principle,decrease in $O_{2}$  will shift the equilibrium towards product side to keep the equilibrium constant unchanged.

(III) Adding a catalyst will not change position of equilibrium. Catalyst only helps to achieve equilibrium in a lesser time.

(IV) As this reaction is an endothermic reaction therefore heat is consumed in formation of product. Therefore increase in temperature will lead to formation of more product to consume excess heat added.

(V) Pure solids and liquids do not affect position of equilibrium as their concentrations remain unchanged.