A sample of air was collected on a day when the total atmosphere pressure was 592 mmHg. The sample contained only oxygen and nitrogen gas. If the oxygen in the sample had a pressure of 261 mmHg, how much pressure did the nitrogen
have? NOTE: You must show your calculation on the attached scratch paper,
including which of the Gas Law formulas you used. *
A. 853 mm Hg
B. 0.206 mm Hg
C. 4.76 mm Hg
D. 331 mm Hg
(Please show your work)

1. The gas law used: Dalton's law of partial pressure.

2. Pressure of nitrogen = 331 mmHg

Explanation:

From the question given above, the following data were obtained:

Total pressure (Pₜ) = 592 mmHg

Pressure of Oxygen (Pₒ) = 261 mmHg

Pressure of nitrogen (Pₙ) =?

The pressure of nitrogen in the sample can be obtained by using the Dalton's law of partial pressure. This is illustrated below:

Pₜ = Pₒ + Pₙ

592 = 261 + Pₙ

Collect like terms

592 – 261 = Pₙ

331 = Pₙ

Pₙ = 331 mmHg

Therefore, the pressure of nitrogen in the sample is 331 mmHg

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