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Question 8.CC.4: A gas mixture with a total pressure of 1.18 atm contains hel......

A gas mixture with a total pressure of 1.18 atm contains helium gas at a partial pressure of 465 mmHg and nitrogen gas. What is the partial pressure, in atmospheres, of the nitrogen gas?

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Initially, we convert the partial pressure of helium gas from mmHg to atm.

465\ \cancel{ mmHg} \times \frac{1\ atm }{760\ \cancel{mmHg} }=0.612\ atm \text { of He gas }

Using Dalton’s law, we solve for the needed quantity, P_{N_{2}} in atm.

\begin{aligned} & P_{\text {total }}=P_{ N _2}+P_{ He } \\ & P_{ N _2}=P_{\text {total }}-P_{ He } \\ & P_{ N _2}=1.18\ atm -0.612\ atm =0.57\ atm \end{aligned}

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