What should be the mole fraction of O2 in the gas mixture the diver breathes in order to have the same partial pressure of oxygen in his lungs as he would at sea level? Note that the mole fraction of oxygen at sea level is 0.209.

The question is incomplete, here is the complete question:

A scuba diver is at a depth of 355 m, where the pressure is 36.5 atm.

What should be the mole fraction of in the gas mixture the diver breathes in order to have the same partial pressure of oxygen in his lungs as he would at sea level? Note that the mole fraction of oxygen at sea level is 0.209.

The mole fraction of oxygen in the gas mixture is 0.00573

Explanation:

To calculate the partial pressure, we use the equation given by Raoult's law, which is:

     ........(1)

where,

= partial pressure of oxygen at sea level = ?

= total pressure at sea level = 1.00 atm

= mole fraction of oxygen at sea level = 0.209

Putting values in equation 1, we get:

As, partial pressure of the oxygen in the diver's lungs is equal to the partial pressure of oxygen at sea level

We are given:

Putting values in equation 1, we get:

Hence, the mole fraction of oxygen in the gas mixture is 0.00573

it's filtration, but this is an assumption so my apologies if i got this