A student determines the mass percent of copper in a bronze alloy sample using an iodometric redox titration. A \(1.000 \text{ g}\) sample of the alloy is dissolved to convert all copper into \(\text{Cu}^{2+}\text{(aq)}\). Excess \(\text{KI(aq)}\) is added, producing solid copper(I) iodide and iodine according to the reaction below:

\[2\text{Cu}^{2+}\text{(aq)} + 4\text{I}^-\text{(aq)} \rightarrow 2\text{CuI(s)} + \text{I}_2\text{(aq)}\]

The liberated \(\text{I}_2\text{(aq)}\) is then titrated with \(0.200 \text{ M } \text{Na}_2\text{S}_2\text{O}_3\text{(aq)}\), requiring \(25.00 \text{ mL}\) of titrant to reach the endpoint according to the reaction below:

\[\text{I}_2\text{(aq)} + 2\text{S}_2\text{O}_3^{2-}\text{(aq)} \rightarrow 2\text{I}^-\text{(aq)} + \text{S}_4\text{O}_6^{2-}\text{(aq)}\]

Based on these results, what is the mass percent of copper in the alloy sample?