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

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.

$p_i=X_i\times p$

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:

$0.300=X_i\times 5.0$

$X_i=\frac{0.300}{5.0}=0.060$

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.