Partial Pressure Calculation

Question

33. A mixture of 0.3 mol of $N_{2}$, 0.5 mol of $CO_{2}$, and 0.4 mol of $O_{2}$ exerts a pressure of 2.4 atm on the walls of the vessel that contains it. What is the pressure exerted by the nitrogen?
A) 0.8 atm
B) 0.6 atm
C) 0.5 atm
D) 0.3 atm
E) 0.75 atm

Solvi · Accepted Answer

Hi Ersan, let's solve this chemistry problem about gas mixtures and partial pressures. We are given a mixture of three gases: nitrogen, carbon dioxide, and oxygen. First, let's list the number of moles for each component. To find the partial pressure of nitrogen, we first need to calculate the total number of moles in the mixture. Plugging in our values, zero point three plus zero point five plus zero point four equals one point two moles in total. Now we can use Dalton's Law of partial pressures. The partial pressure of a gas is its mole fraction multiplied by the total pressure.

Partial Pressure Calculation

Animated Video Solution

Step by Step Written Solution