State the test for oxygen gas and the observation.
State how the graph in Fig. 4.1 shows the rate of reaction at time $t_2$ is lower than at time $t_1$.
Explain, using collision theory, why the rate of reaction at time $t_2$ is lower than at time $t_1$.
On Fig. 4.1, sketch the graph obtained when the experiment is repeated using aqueous hydrogen peroxide at a higher temperature. All other conditions remain unchanged.
Calculate the concentration of the aqueous hydrogen peroxide in g/dm$^3$ by following these steps: • Work out the amount of oxygen gas produced in moles. • Find the amount of hydrogen peroxide that reacts in moles. • Work out the concentration of aqueous hydrogen peroxide in mol/dm$^3$. • Work out the concentration of aqueous hydrogen peroxide in g/dm$^3$.
Suggest the identity of one other metal oxide that also catalyses this reaction.