CO (5.00 g)and CO₂ (5.00 g)were placed in a 750.0 mL container at 50.0 °C.The partial pressure of CO₂ in the container was ________ atm.

Question

Quizplus · Accepted Answer

The partial pressure of a gas is equal to the mole fraction of that gas multiplied by the total pressure. The mole fraction of CO2 is equal to the number of moles of CO2 divided by the total number of moles of gas in the container. The number of moles of CO2 is equal to the mass of CO2 divided by the molar mass of CO2. The molar mass of CO2 is 44.01 g/mol. The number of moles of CO is equal to the mass of CO divided by the molar mass of CO. The molar mass of CO is 28.01 g/mol. The total number of moles of gas in the container is equal to the number of moles of CO plus the number of moles of CO2. The total pressure is equal to the sum of the partial pressures of the two gases. The partial pressure of CO2 is equal to the mole fraction of CO2 multiplied by the total pressure. The mole fraction of CO2 is equal to 5.00 g / (5.00 g + 5.00 g) = 0.500. The total pressure is equal to 1 atm. The partial pressure of CO2 is equal to 0.500 atm * 1 atm = 0.500 atm.

CO (500 G)and CO2 (5

CO (500 G)and CO₂ (5