1. The problem statement, all variables and given/known data 0.2500 g sample of an Aℓ-Zn alloy reacts with HCℓ to form hydrogen gas: Aℓ(s) + 3H+(aq) → Aℓ3+(aq) + 3/2H2(g) Zn(s) + 2H+(aq) → Zn2+(aq) + H2(g) The hydrogen produced has a volume of 0.147 L at 25°C and 755 mm Hg. What is the percentage of zinc in the alloy? 2. Relevant equations PV=NRT 3. The attempt at a solution Frist I start out finding the number of moles of Hydrogen gas produced by using PV=NRT N=((.993atm)(.147L))/((.0821)(298K))= .00596 mol of H2 1mol of Al = 26.98g 1mol of Zn = 65.93g now what should I do? Help please.