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Zinc metal is added to hydrochloric acid to generate hydrogen gas, which is collected over a liquid whose vapor pressure is the same as pure water at 20.0°C (18 torr). The volume of the gas mixture is 1.7 L and its total pressure is 0.810 atm. Determine the partial pressure of the hydrogen gas in this mixture.

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Answer:

The partial pressure of the hydrogen gas is 0.786 atm

Explanation:

In this case, the gas mixture contains the vapor from the liquid, and hydrogen gas. Before we do any calculations, we need to convert 18 torr into atm:

[tex]18torr*\frac{1atm}{760torr} =0.0237atm[/tex]

Then we use the equation of Dalton's law, which states that the total pressure of a gas mixture is equal to the sum of the partial pressure of its components:

[tex]P_{T}=P_{H}+P_{v}[/tex]

Where [tex]P_{T}[/tex] is the total pressure, [tex]P_{H}[/tex] is the partial pressure of hydrogen, and [tex]P_{v}[/tex] is the partial pressure of the vapor of the liquid.

Replacing the data we know:

0.810 atm= [tex]P_{H}[/tex] + 0.0237 atm

[tex]P_{H}[/tex]= 0.786 atm

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