A sample of oxygen is collected over water at a total pressure of 592.2 mmHg at 27C. The vapor pressure of water at 27C is 26.7 mmHg. What is the partial pressure of O2?


***Please show steps

Dalton's Law of partial pressure tells us that Ptotal = pO2 + pH2O.

How do you find pressure in this case ?

To find the partial pressure of O2, we need to subtract the vapor pressure of water from the total pressure.

Step 1: Subtract the vapor pressure of water from the total pressure:
Partial pressure of O2 = Total pressure - Vapor pressure of water
= 592.2 mmHg - 26.7 mmHg

Step 2: Calculate the partial pressure of O2:
Partial pressure of O2 = 565.5 mmHg

Therefore, the partial pressure of O2 is 565.5 mmHg.

Read the problem.

Ptotal = 592.2 mm
pO2 = 26.7 mm
You're making this a lot harder than it is.
592.2 = 26.7 + pO2
pO2 = 592.2-26.7 = ?