A sealed vessel contains 1.47 moles of oxygen, 5.29moles of carbon dioxide, and 4.14 moles of nitrogen gas. The total pressure of the gas mixture is 7.7 atmospheres. What is the partial pressure of the carbon dioxide?
Question
A sealed vessel contains 1.47 moles of oxygen, 5.29moles of carbon dioxide, and 4.14 moles of nitrogen gas. The total pressure of the gas mixture is 7.7 atmospheres. What is the partial pressure of the carbon dioxide?
Solution
To find the partial pressure of carbon dioxide, we first need to find the total number of moles of gas in the vessel.
Step 1: Add up all the moles of gas 1.47 moles (Oxygen) + 5.29 moles (Carbon Dioxide) + 4.14 moles (Nitrogen) = 10.9 moles (Total)
Step 2: Calculate the mole fraction of carbon dioxide Mole fraction = moles of component / total moles Mole fraction (Carbon Dioxide) = 5.29 moles (Carbon Dioxide) / 10.9 moles (Total) = 0.485
Step 3: Calculate the partial pressure of carbon dioxide Partial pressure = mole fraction * total pressure Partial pressure (Carbon Dioxide) = 0.485 * 7.7 atm = 3.73 atm
So, the partial pressure of the carbon dioxide is 3.73 atmospheres.
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