Answer:
The partial pressures of Oâ‚‚ and COâ‚‚ are 0.489 atm and 0.511 atm respectively.
Explanation:
From the Questions we are given;
Volume = 10 Liter
Temperature = 298 K
Pressure = 1 atm
We need to calculate the partial pressures of Oâ‚‚ and COâ‚‚
Step 1 : Number of moles of gaseous mixture
Using the ideal gas equation;
PV =nRT, where P is the pressure, V is the volume, n is the number of moles, T is the temperature in K and R is the ideal gas constant (0.082 L∙atm/K∙mol)
Therefore;
[tex]n =\frac{PV}{RT}[/tex]
[tex]n = \frac{(10)(1)}{(298)(0.082)}[/tex]
Solving for n
[tex]n = 0.409 moles[/tex]
Step 2: Moles of COâ‚‚
Total number of moles of the mixture = 0.409 moles
Moles of Oxygen = 0.2 moles
Therefore;
Moles of COâ‚‚ = 0.409 moles - 0.2 moles
           = 0.209 moles
Step 3: Partial pressures of Oâ‚‚ and COâ‚‚
[tex]Partial pressure = \frac{No. of moles}{Total number of moles}(total pressure)[/tex]
Therefore;
Partial pressure of Oxygen gas
[tex]= \frac{number of moles of Oxygen}{Total number of moles} (Total pressure)[/tex]
[tex]= \frac{0.2}{0.409}(1)\\= 0.489 atm[/tex]
Partial pressure of COâ‚‚
[tex]= \frac{number of moles of COâ‚‚}{Total number of moles} (Total pressure)[/tex]
[tex]= \frac{0.209}{0.409}(1)\\= 0.511 atm[/tex]
Thus, the partial pressures of Oâ‚‚ and COâ‚‚ are 0.489 atm and 0.511 atm respectively.
