Answer:
The total pressure of the gas mixture = 2.76 atm
Note: The question is not complete. The complete question is as follow:
If 43.1 g of O2 and 6.8 g of CO2 are placed in a 13.7 L container at 34 degree Celsius , what is the pressure of the mixture of gases?
Explanation:
Mass of O₂ gas = 43.1 g, molar mass of O₂ gas = 32.0 g/mol
Number of moles of O₂ gas = 43.1/32.0 = 1.347 moles
Mass of CO₂ gas = 6.8 g, molar mass of CO₂ gas = 44.0 g
Number of moles of CO₂ gas = 6.8/44 = 0.155 moles
Total number of moles of gas mixture, n = (1.347 + 0.155) = 1.502 moles
Volume of gas mixture, V = 13.7 L
Temperature of gas mixture, T = 34 °C = (273.15 + 34) K = 307.15 K
Pressure of gas mixture = ?
Molar gas constant, R = 0.0821 liter·atm/mol·K.
Using the ideal gas equation: PV =nRT
P = nRT/V
P = (1.502 × 0.0821 × 307.15) / 13.7
P = 2.76 atm
Therefore, the total pressure of the gas mixture = 2.76 atm
