**Calculate the ****no. of moles of H _{2} using the ideal gas equation:**

**Given: **

**• ****P _{H2 }**= 738 torr (

1 atm = 760 torr

${\mathit{P}}_{{\mathbf{H}}_{\mathbf{2}}}\mathbf{=}\mathbf{738}\mathbf{}\overline{)\mathbf{torr}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{a}\mathbf{t}\mathbf{m}}{\mathbf{760}\mathbf{}\overline{)\mathbf{torr}}}$

${\mathit{P}}_{{\mathbf{H}}_{\mathbf{2}}}\mathbf{=}$**0.971 atm**

**• V** = 160 mL (**L **is needed in the ideal gas equation: convert from mL to L)

1 mL = 10^{-3} L

${\mathit{V}}_{{\mathbf{H}}_{\mathbf{2}}}\mathbf{=}\mathbf{160}\mathbf{}\overline{)\mathbf{m}\mathbf{L}}\mathbf{\times}\frac{{\mathbf{10}}^{\mathbf{-}\mathbf{3}}\mathbf{}\mathbf{L}}{\mathbf{1}\mathbf{}\overline{)\mathbf{m}\mathbf{L}}}$

${\mathit{V}}_{{\mathbf{H}}_{\mathbf{2}}}\mathbf{=}$**0.160 L**

• **T** = 24.0°C *( K is need in the ideal gas equation: convert from *

T = 24.0°C + 273.15**T = 297.15 K**

• **R** = gas constant = **0.08206 (L****∙atm)/(mol****∙K)**

Hydrogen gas is produced when zinc reacts with sulfuric acid:

Zn(s) + H_{2}SO_{4}(aq) → ZnSO_{4}(aq) + H_{2}(g)

If 160 mL of wet H_{2} is collected over water at 24 ^{o}C and a barometric pressure of 738 torr, how many grams of Zn have been consumed? (The vapor pressure of water is 22.38 torr.)

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