What is the partial pressure of carbon dioxide in a container that contains 3.63 mol of oxygen, 1.49 mol of nitrogen, and 4.49 mol of carbon dioxide when the total pressure is 871 mmHg?

Partial pressure of CO₂ is 406.9 mmHg

Explanation:

To solve the question we should apply the concept of the mole fraction.

Mole fraction = Moles of gas / Total moles

We have the total moles of the mixture, if we have the moles for each gas inside. (3.63 moles of O₂, 1.49 moles of N₂ and 4.49 moles of CO₂)

Total moles = 3.63 mol O₂ + 1.49 mol N₂ + 4.49 mol CO₂ = 9.61 moles

To determiine the partial pressure of CO₂ we apply

Mole fraction of CO₂ → mol of CO₂ / Total moles = P. pressure CO₂ / Total P

Partial pressure of CO₂ = (mol of CO₂ / Total moles) . Total pressure

We replace values: (4.49 moles / 9.61 moles) . 871 mmHg = 406.9 mmHg

Partial pressure O2 = 329 mmHg

Partial pressure N2 = 135 mmHg

Partial pressure CO2 = 407 mmHg

Explanation:

Step 1: Data given

Number of moles oxygen (O2) = 3.63 moles

Number of moles nitrogen (N2) = 1.49 moles

Number of moles carbon dioxide (CO2) = 4.49 moles

Total pressure = 871 mmHg

Step 2: Calculate total number of moles

Total moles = moles O2 + moles N2 + moles CO2

Total moles = 3.63 + 1.49 + 4.49

Total moles =  9.61 moles

Step 3: Calculate the mol ratio

Mol ratio number of moles compound / total moles

Mol ratio O2 = 3.63 moles / 9.61 moles

Mol ratio O2 = 0.378

Mol ratio N2 = 1.49 moles / 9.61 moles

Mol ratio N2 = 0.155

Mol ratio CO2 = 4.49 moles / 9.61 moles

Mol ratio CO2 = 0.467

Step 4: Calculate partial pressure

Partial pressure = mol ratio * total pressure

Partial pressure O2 = 0.378 * 871 mmHg

Partial pressure O2 = 329 mmHg

Partial pressure N2 = 0.155 * 871mmHg

Partial pressure N2 = 135 mmHg

Partial pressure CO2 = 0.467 * 871 mmHg

Partial pressure CO2 = 407 mmHg

i think   the answer is c hope i'm right