Respuesta :
Answer:
0.85 atm
Explanation:
We start by getting the total number of moles of all gases.
Total moles = 0.220 + 0.350 + 0.640 = 1.21 mol
Then we get the fraction of Oxygen moles and multiply by the total pressure;
The pressure of O2 = 0.350 mol / 1.21 mol x 2.95 atm
= 0.85 atm
Answer:
Partial pressure of O2 = 0.875 atm
Explanation:
Given:
Moles of Radon gas (Rn) =0.220
Moles of O2 gas = 0.350
Moles of argon gas (Ar) = 0.640
Total pressure = 2.95 atm
To determine:
The partial pressure of O2
Explanation:
As per Dalton's Law, the total pressure exerted by a mixture of gases is equal to the sum of their partial pressures.
Here:
[tex]P(total) = P(Rn) + P(O2) + P(Ar)\\\\where \ the\ partial\ pressure \ is \ given\ as:\\\\partial pressure = mole fraction * total pressure\\\\P(O2) = mole fraction (O2) *P(total)\\\\P(O2) = \frac{moles\ O2}{total\ moles}*P(total)\\ \\P(O2) = \frac{0.350}{1.18} * 2.95=0.875 atm[/tex]
