A student performs a gravimetric analysis to determine the mass percent of silver in an alloy. A \(2.00 \text{ g}\) sample of the alloy is completely dissolved in excess concentrated \(\text{HNO}_3\text{(aq)}\). An excess of \(\text{NaCl(aq)}\) is added to the solution, causing all of the silver to precipitate as \(\text{AgCl(s)}\). The precipitate is collected on filter paper, washed, and dried to constant mass. The experimental data and molar masses are shown in the tables below.

Measurement	Mass
Mass of alloy sample	\(2.00 \text{ g}\)
Mass of dry filter paper	\(0.800 \text{ g}\)
Mass of filter paper \(+\) dry \(\text{AgCl(s)}\)	\(2.235 \text{ g}\)

Substance	Molar Mass (\(\text{g/mol}\))
\(\text{Ag}\)	\(108.0\)
\(\text{Cl}\)	\(35.5\)
\(\text{AgCl}\)	\(143.5\)

Based on the data, what is the mass percent of \(\text{Ag}\) in the alloy sample?