A sample of oxygen is collected over water at a total pressure of 692.2 mmHg at 17°C. The vapor pressure of water at 17°C is 14.5 mmHg. The partial pressure of the O2

677.7 mmHg

Explanation:

This is Dalton's law, where you add each partial pressure into total.

You are given total pressure of 692.2 mmHg

Partical pressure of water is: 14.5 mmHg

To find the partial pressure of O2, you subtract the total pressure and the given vapor pressure of water.

If you want the answer in atm, it would be: 0.892 atm

677.7 mmHg X (1 atm/760 mmHg) = 0.892 atm

Hope this helps!

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