If oxygen were collected over water at 293 K and the

totalpressure of the wet gas were 670 mmHg, what would be the

partialpressure of the oxygen?

Question

Chemistry

Chanel Campbell

18 July, 02:53

If oxygen were collected over water at 293 K and the

totalpressure of the wet gas were 670 mmHg, what would be the

partialpressure of the oxygen?

+4

Answers (1)

Know the Answer?

Jensen Baxter · Answer 1

652 mmHg

Explanation:

Given data

Total pressure (P) : 670 mmHg Temperature (T) : 293 K Vapor pressure of water at 293 K (Pwater) : 17.54 mmHg

When oxygen is collected over water, the total pressure is the sum of the partial pressures of oxygen and water vapor at the given temperature.

P = Poxygen + Pwater

Poxygen = P - Pwater

Poxygen = 670 mmHg - 17.54 mmHg

Poxygen = 652 mmHg

If oxygen were collected over water at 293 K and thetotalpressure of the wet gas were 670 mmHg, what would be thepartialpressure of the oxygen?

If oxygen were collected over water at 293 K and the

totalpressure of the wet gas were 670 mmHg, what would be the

partialpressure of the oxygen?