Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation:

$2Al(s)+2$NaOH$(aq)+6H_{2}O(l)2$NaAl$(OH{)}_4(aq)+3H_2(g)$

The product gas, $H_2,$ is collected over water at a temperature of $25C$ and a pressure of $748\mathrm{.}0mmHg.$ If the wet $H_2$ gas formed occupies a volume of $5\mathrm{.}16L,$ the number of grams of $H_2$ formed is water is $23\mathrm{.}8mmHg$ at $25C.$

g$.$ The vapor pressure of

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