Methanol has tremendous potential to be used as an alternate fuel. Carbon monoxide gas reacted with hydrogen gas can be used to produce methanol.

A student reacted $37\mathrm{.}8g$ of $H_{2(g)}$ with excess $C{O}_{(g)}$ to produce methanol.

If his percent yield was $47\mathrm{.}7\%,$ calculate the mass $($in $g)$ of $C{H}_{3}O{H}_{(0)}$ that he collected in the experiment

Hint Write a balanced chemical reaction equation.