Chemistry College

A 300.0 mL quantity of hydrogen is collected over water at 19.5 C and a total atmospheric pressure of 750. mm Hg. The partial pressure of water at this temperature is 17.0 mm Hg

Answers

Answer 1

The partial pressure of hydrogen in the collected gas sample is 733.0 mm Hg (calculated by subtracting the partial pressure of water, 17.0 mm Hg, from the total atmospheric pressure, 750.0 mm Hg).

When a gas is collected over water, the presence of water vapor affects the total pressure observed. In this case, the total atmospheric pressure is given as 750.0 mm Hg, and the partial pressure of water vapor at 19.5°C is 17.0 mm Hg.

To determine the partial pressure of hydrogen, we need to subtract the partial pressure of water vapor from the total atmospheric pressure. Partial pressure refers to the pressure exerted by an individual gas component in a mixture. In this scenario, the collected gas is primarily hydrogen, with water vapor being the other component.

By subtracting the partial pressure of water vapor (17.0 mm Hg) from the total atmospheric pressure (750.0 mm Hg), we can find the partial pressure of hydrogen:

Partial pressure of hydrogen = Total atmospheric pressure - Partial pressure of water vapor

Partial pressure of hydrogen = 750.0 mm Hg - 17.0 mm Hg

Partial pressure of hydrogen = 733.0 mm Hg

Therefore, the partial pressure of hydrogen in the collected gas sample is 733.0 mm Hg.

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