A sample of gas is collected by water displacement. The atmospheric pressure in the room is 757mmHg and the vapor pressure of water is 17.5mmHg. What is the partial pressure of hydrogen under these conditions?

ptotal = pH2 + pH2O

ptotal = 757
pH2O = 17.5
pH2 = ? Substitute and solve.

To determine the partial pressure of hydrogen under these conditions, you need to subtract the vapor pressure of water from the atmospheric pressure.

Partial pressure of hydrogen = Atmospheric pressure - Vapor pressure of water

Given that the atmospheric pressure is 757 mmHg and the vapor pressure of water is 17.5 mmHg, you can calculate the partial pressure of hydrogen as follows:

Partial pressure of hydrogen = 757 mmHg - 17.5 mmHg

Partial pressure of hydrogen = 739.5 mmHg

Therefore, the partial pressure of hydrogen under these conditions is 739.5 mmHg.

To find the partial pressure of hydrogen, we need to subtract the vapor pressure of water from the total atmospheric pressure.

Step 1: Subtract the vapor pressure of water from the atmospheric pressure.
757 mmHg - 17.5 mmHg = 739.5 mmHg

Therefore, the partial pressure of hydrogen under these conditions is 739.5 mmHg.