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.
[tex]p_i=X_i\times p[/tex]
where [tex]p_i[/tex] = partial pressure of gas = 0.300 atm
[tex]X_i[/tex] = mole fraction of the component = ?
p = total pressure = 5.0 atm
Putting in the values we get:
[tex]0.300=X_i\times 5.0[/tex]
[tex]X_i=\frac{0.300}{5.0}=0.060[/tex]
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.
