Question

Assume a scuba diver is working at a depth where the total pressure is 5.0 atm (about 50 m below the surface). What mole fraction of oxygen is necessary in order for the partial pressure of oxygen in the gas mixture the diver breathes to be 0.300 atm?

Answer 1

Answer: 0.060

Step-by-step explanation:

According to the Dalton's Law, the partial pressure exerted by component 'i' in a gas mixture is equal to the product of the mole fraction of the component and the total pressure.

`p_i=X_i* p`

where
`p_i` = partial pressure of gas = 0.300 atm

`X_i` = mole fraction of the component = ?

p = total pressure = 5.0 atm

Putting in the values we get:

`0.300=X_i* 5.0`

`X_i=(0.300)/(5.0)=0.060`

Thus mole fraction of oxygen is necessary in order for the partial pressure of oxygen in the gas mixture the diver breathes to be 0.300 atm is 0.060.