Question

If anybody sees this can they help me out?

At a depth of 50 m, the pressure is 512 kPa (kilopascals).
A diver breathing air (78% N2, 21% O2) at this depth would have what partial pressure of oxygen in his lungs?

A) 404 kPa
B) 5.1 kPa
C) 108kPa
D) 512 kPa


At 273 K, you collect 0.5 L of oxygen over water that has a total pressure of 22 kPa.
What is the partial pressure of oxygen?
(The partial pressure of water vapor at 273 K is 0.61 kPa .)

A) 36.07 kPa
B) 21.39 kPa
C) 273.61 kPa
D) 22.61 kPa


You breathe in 12.0 L of pure oxygen at 298 K and 1,000 kPa to fill your lungs.
How many moles of oxygen did you take in?
Use the ideal gas law: PV = nRT where R=8.31 L*kPa/mol*K

A) 0.05 mole
B) 1.21 moles
C) 2.42 moles
D) 4.84 moles

Answer 1

A) The partial pressure of oxygen in the diver's lungs would be 108 kPa.

B) The partial pressure of oxygen would be 21.39 kPa.

C) The number of moles of oxygen taken in would be 2.42 moles.

Step-by-step explanation:

Answer 2

A) The partial pressure of oxygen in the diver's lungs would be 108 kPa.
B) The partial pressure of oxygen would be 21.39 kPa.
C) The number of moles of oxygen taken in would be 2.42 moles.