HELP!!!A problem on quantitative aspects of electrolysis 1. The problem statement, all variables and given/known data A quantity of electric charge brings about the deposition of 3.34 g Cu at a cathode during the electrolysis of a solution containing Cu2+(aq). What volume of H2(g) measured at 27.8oC and 767 mmHg, would be produced by this same quantity of electric charge in the reduction of H+(aq) at a cathode? 3. The attempt at a solution I don't really know the formula for solving the volume in the electrolysis. The way I approached this problem is by using the ideal gas law(but I don't think it is the right way): PV=nRT 2H++2e--->H2(g) we are trying to solve for V, so V=? P=767mmHg R=62.36367L·mmHg·K−1·mol−1 n=2 T=300.95K plug the numbers into the equation and I got V=48.94L Can someone please help me with it? Is it the right way for solving the problem? thank you very much.