A student investigates the kinetics of the reaction between solid calcium carbonate and hydrochloric acid, represented by the balanced equation below:

\[\text{CaCO}_3\text{(s)} + 2\text{HCl(aq)} \rightarrow \text{CaCl}_2\text{(aq)} + \text{H}_2\text{O(l)} + \text{CO}_2\text{(g)}\]

In Trial 1, the student adds a single \(2.0 \text{ g}\) chip of \(\text{CaCO}_3\text{(s)}\) to \(50.0 \text{ mL}\) of \(1.0 \text{ M HCl(aq)}\) at \(25^\circ\text{C}\) and measures the initial rate of \(\text{CO}_2\text{(g)}\) production. In Trial 2, the student repeats the experiment using \(2.0 \text{ g}\) of finely powdered \(\text{CaCO}_3\text{(s)}\) with \(50.0 \text{ mL}\) of \(1.0 \text{ M HCl(aq)}\) at \(25^\circ\text{C}\). Which of the following best predicts and explains the effect of using powdered \(\text{CaCO}_3\text{(s)}\) on the initial reaction rate?