Magnesium carbonate undergoes reaction with dilute hydrochloric acid.
$\text{MgCO}_3(s) + 2\text{HCl}(aq) \rightarrow \text{MgCl}_2(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g)$
A surplus of magnesium carbonate pieces was introduced into dilute hydrochloric acid. The equipment shown in the diagram was used to measure the volume of gas given off. The total volume of gas gathered was noted every 20 seconds.
(a(i))[4]
Describe how the rate of this reaction altered as the reaction proceeded. Explain why the rate changed in this way.
(a(ii))[4]
Explain how the initial rate of reaction and total volume of gas collected would compare with the first experiment.
(b)[5]
Explain why the reaction rate increased.
Worked solution & mark scheme
This 13-mark question has a full step-by-step worked solution and mark scheme. One marking point: “the reaction became slower” …