Respuesta :
We know that a gas mixture contains 79% nitrogen and 21% oxygen. We must find the partial pressures if the total pressure is 1.02 atm.
In order to find the partial pressures we must use the next equation
[tex]\bar{P}=x_i\cdot P_{total}[/tex]Where,
[tex]\begin{gathered} x_i\text{ represents the }molar\text{ fraction} \\ P_{total}\text{ represents the total pressure} \end{gathered}[/tex]1. For nitrogen which is in a 79%
[tex]x_i=79\text{ \%}=\frac{79}{100}=0.79[/tex]Now, replacing in the formula for the partial pressure
[tex]\bar{P_N}=0.79\cdot1.02\text{atm}=0.8058\text{atm}[/tex]2. For oxygen which is in a 21%
[tex]x_i=21\text{ \%}=\frac{21}{100}=0.21[/tex]Now, replacing in the formula for the partial pressure
[tex]\bar{P}_O=0.21\cdot1.02atm=0.2142atm[/tex]ANSWER:
- The partial pressure of the nitrogen is 0.8058 atm.
- The partial pressure of the oxygen is 0.2142 atm.
