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**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 Cu

^{2+}(aq).

What volume of H

_{2}(g) measured at 27.8

^{o}C 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

^{-}-->H

_{2}(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.