1. The problem statement, all variables and given/known data An alloy of copper and silver weighing 0.5000 grams is dissolved in HNO3 and treated with H2S to precipitate both CuS and Ag2S. It is found that the solid sulphides weigh 0.7300 grams. Calculate the percentage of Ag in the alloy. (12.9 %) 2Ag+(aq) + H2S(aq)→ Ag2S(s) + 2H+(aq) Cu+2(aq) + H2S(aq)→ CuS(s) + 2H+(aq) 2. Relevant equations mass of Ag/mass of alloy = % of Ag 3. The attempt at a solution I'm not too sure how to start this question… So far, I have 0.7300 g Ag2S x 1 mol / 215.74 g Ag2 = 2.945 x 10-3 mol Ag2S 2.945 x 10-3 mol Ag2S x 215.74 g Ag2/ 1 mol Ag2S = 0.6353 g Ag2 I'm not sure if I'm on the right track here?