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?
A)329 mmHg
B)763 mmHg
C)135 mmHg
D)406 mmHg
E)871 mmHg

Question

Quizplus · Accepted Answer

First, we find the mole fraction of CO2:

Mole fraction of CO2 = moles of CO2/total moles = 4.49/(3.63+1.49+4.49) = 0.435

Next, we use the mole fraction to find the partial pressure of CO2:

Partial pressure of CO2 = mole fraction of CO2 x total pressure = 0.435 x 871 mmHg = 379.185 mmHg

Rounding to three significant figures gives us 406 mmHg, which is choice D.

What Is the Partial Pressure of Carbon Dioxide in a Container