A sample of NaNO3 was fully decomposed into its elements, and the resulting gas was collected over water at 34°C. If the total pressure of the collected gas was 760 torr, and the vapor pressure of water at 34°C is 40.0 torr, what was the partial pressure of N2 gas in the flask?

Question

Jayson Kirby

Chemistry

22 March, 10:34

A sample of NaNO3 was fully decomposed into its elements, and the resulting gas was collected over water at 34°C. If the total pressure of the collected gas was 760 torr, and the vapor pressure of water at 34°C is 40.0 torr, what was the partial pressure of N2 gas in the flask?

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Answers (1)

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Cindy Riggs · Answer 1

Answer is: the partial pressure of nitrogen gas is 720.0 torr.

The total pressure of an ideal gas mixture is the sum of the partial pressures of the gases in the mixture.

p (mixture) = p (water) + p (nitrogen).

p (water) = 40.0 torr; partial pressure of the water.

p (nitrogen) = p (mixture) - p (water).

p (nitrogen) = 760.0 torr - 40.0 torr.

p (nitrogen) = 720.0; patial pressure of N₂.