1. The problem statement, all variables and given/known data Determine how many grams of Mg must react with HCl in order to produce 40 mL of hydrogen gas at 22 degrees Celsius and 1.02 bar. Also, If the Mg ribbon weighs 0.836 mg/mm, how many mm of the ribbon will you require? 2. Relevant equations PV=nRT Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) 3. The attempt at a solution n=PV/RT n= (1.00 atm)(0.04 L) / (0.0821 L*atm/mol*K)(295.15 K) n= 0.04/24.232 = 0.0016507098 mol * 24.3050 g/mol = 0.040 g Mg 40 mg x 1mm / 0.836mg = 47.85mm Correct? Thanks for the help!