Question

some n₂ gas is mixed with some o₂ gas, and the sketch below shows a representative sample of the mixture. the total pressure of the mixture is measured, and found to be 1.50 atm.
calculate the mole fraction and partial pressure of each gas in this mixture. round your answers to 3 significant digits. you may assume each gas behaves as an ideal gas.

Explanation:

Step1: Count the number of each gas molecule

There are 10 blue ($\ce{N2}$) molecules and 8 red ($\ce{O2}$) molecules. The total number of molecules \(n_{total}=10 + 8=18\).

Step2: Calculate the mole fraction

The mole fraction formula is \(x_i=\frac{n_i}{n_{total}}\).
For \(\ce{N2}\): \(x_{N_2}=\frac{10}{18}\approx0.556\).
For \(\ce{O2}\): \(x_{O_2}=\frac{8}{18}\approx0.444\).

Step3: Calculate the partial pressure

The partial - pressure formula is \(P_i = x_iP_{total}\). Given \(P_{total}=1.50\space atm\).
For \(\ce{N2}\): \(P_{N_2}=x_{N_2}\times P_{total}=0.556\times1.50 = 0.834\space atm\).
For \(\ce{O2}\): \(P_{O_2}=x_{O_2}\times P_{total}=0.444\times1.50=0.666\space atm\).

Answer:

gas	mole fraction	partial pressure
\(\ce{N2}\)	\(0.556\)	\(0.834\space atm\)