${\mathbf{P}}_{\mathbf{total}}\mathbf{=}{\mathbf{P}}_{{\mathbf{H}}_{\mathbf{2}}}\mathbf{+}{\mathbf{P}}_{{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}$

$\mathbf{1}\mathbf{.}\mathbf{032}\mathbf{}\mathbf{atm}\mathbf{=}{\mathbf{P}}_{{\mathbf{H}}_{\mathbf{2}}}\mathbf{+}\mathbf{32}\mathbf{}\overline{)\mathbf{torr}}\left(\frac{1\mathrm{atm}}{760\overline{)\mathrm{torr}}}\right)\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\mathbf{1}\mathbf{.}\mathbf{032}\mathbf{}\mathbf{atm}\mathbf{=}{\mathbf{P}}_{{\mathbf{H}}_{\mathbf{2}}}\mathbf{+}\mathbf{0}\mathbf{.}\mathbf{0421}\mathbf{}\mathbf{atm}$

Small quantities of hydrogen gas can be prepared in the laboratory by the addition of aqueous hydrochloric acid to metallic zinc.

Zn(*s*) + 2HCl(*aq*) → ZnCl_{2}(*aq)* + H_{2}(*g*)

Typically, the hydrogen gas is bubbled through water for collection and becomes saturated with water vapor. Suppose 240. mL of hydrogen gas is collected at 30.°C and has a total pressure of 1.032 atm by this process. What is the partial pressure of hydrogen gas in the sample? How many grams of zinc must have reacted to produce this quantity of hydrogen? (The vapor pressure of water is 32 torr at 30°C.)

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