1. The problem statement, all variables and given/known data 3.50 g of magnesium metal is added to 100. mL of 2.00 M aqueous hydrochloric acid. The substances react to completion, producing aqueous magnesium chloride and hydrogen gas (H2). How many liters of pure hydrogen gas, measured at 0.00oC and 1.00 atm are produced in this reaction? 2. Relevant equations PV=nRT 3. The attempt at a solution Rxn Eq: 2Mg + 2HCl --> 2MgCl + H2 3.5 g Mg x (1 mol/24.3g) = .144 mol Mg 2 mol/L HCl x .1L = .2 mol HCl Mg is limiting reactant .144 mol Mg x (1 mol H2/2 mol Mg) = .072 mol H2 V=(nRT)/P=[(.072)(.08206)(273)] / 1 = 1.61 L H2 It says the answer is 2.24L?