A chemist monitors the rate of decomposition of a hydrogen peroxide solution:
2H2O2(aq)→2H2O(l)+O2(g) 2\text{H}_2\text{O}_2(\text{aq}) \rightarrow 2\text{H}_2\text{O}(\text{l}) + \text{O}_2(\text{g}) 2H2O2(aq)→2H2O(l)+O2(g)When the temperature of the reactant solution is raised from 20 ∘C20\text{ }^\circ\text{C}20 ∘C to 35 ∘C35\text{ }^\circ\text{C}35 ∘C, the rate of oxygen gas production increases significantly.
Explain, in terms of particles and collision theory, why increasing the temperature increases the rate of this reaction.
