The combustion of butane $(C_4{H}_{10})$ produces $C{O}_2$ and $H_{2}O$ according to the following balanced equation:

$2C_4{H}_{10}(g)+13O_2(g)8C{O}_2(g)+10H_{2}O(g)$

If the hydrocarbon is present in excess, what mass of water $(H_{2}O)$ in grams will form when $72\mathrm{.}3g$ of $O_2$ react completely?

Round your answer to $3$ sig figs.

$31\mathrm{.}3$

$62\mathrm{.}6$

$52\mathrm{.}9$

$19\mathrm{.}6$

$12\mathrm{.}7$