A student conducts an experiment to determine the composition of a bronze alloy containing only \(\text{Cu}\) and \(\text{Sn}\). A \(2.46 \text{ g}\) sample of the alloy is dissolved completely in excess concentrated \(\text{HNO}_3\text{(aq)}\). During the reaction, all of the tin is oxidized to insoluble hydrated tin(IV) oxide, while the copper dissolves to form \(\text{Cu}^{2+}\text{(aq)}\). The precipitate is collected by filtration, washed, and heated to constant mass in a crucible to yield anhydrous \(\text{SnO}_2\text{(s)}\). The student records the laboratory data in the table below.

Measurement	Value
Mass of bronze alloy sample	\(2.46 \text{ g}\)
Mass of empty crucible and cover	\(18.50 \text{ g}\)
Mass of crucible, cover, and \(\text{SnO}_2\text{(s)}\) after heating	\(20.01 \text{ g}\)
Molar mass of \(\text{Cu}\)	\(63.5 \text{ g/mol}\)
Molar mass of \(\text{Sn}\)	\(119 \text{ g/mol}\)
Molar mass of \(\text{SnO}_2\)	\(151 \text{ g/mol}\)

Based on the data in the table, what is the mole fraction of \(\text{Cu}\) in the bronze alloy sample?