A solution containing both Ag^{+}(aq) and Cu^{2+}(aq) is electrolyzed with a constant current of 0.500 A for 3.00 h. Because Ag^{+} is reduced before Cu^{2+}, 1.50 g of silver is deposited first, after which any remaining charge reduces Cu^{2+} to copper metal. Assuming F=9.65×104C mol−1, what additional mass of copper is deposited during the 3.00 h period? (Molar masses: Ag = 107.9 g mol^{–1}, Cu = 63.55 g mol^{–1})
a) 2.68g
b) 1.34g
c) 0.67g
d) 1.78g