Positive Physics - HELP!!!!

Question

A mixture of 3.31 mol of nitrogen and 4.59 mol of fluorine is in a container. The nitrogen has a partial pressure of 0.737atm. What are the moles of gas? mole fraction of mixture and partial pressure (atm) for Nitrogen, fluorine, and total mixture. What is the partial pressure of the fluorine in the mixture? What is the total pressure of the mix?

Answer 1

We will be applying Dalton's Law of Partial Pressures. According to this law, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the individual gases.

Step 1: Find the total moles of gas. Total moles = moles of nitrogen gas + Fluorine gas

Total moles = 3.31 mol + 4.59 mol = 7.90 mol

Step 2: Calculate the mole fraction of each component.

Mole fraction = moles of each component/ total moles

Mole fraction Nitrogen = moles Nitrogen/total moles = 3.31/7.90 = 0.42 mol N₂

Mole Fraction F = moles F/total moles = 4.59/ 7.90 = 0.581 mol F₂

*NOTE: Nitrogen and fluorine are diatomic elements, meaning they exist in pairs.

Step 3: Find the partial pressures of each element using total pressure equation

P_total = P_N2 + P_F2

The partial pressure of Nitrogen is already given: 0.737 atm

P_F2 = mole fraction F₂ x total pressure

We know the mole fraction of F₂ = 0.581 mol.

Plug P_F2 into P_total equation

P_total = 0.737 atm + (0.581 x P_total )

Try to get P_total to one side of the equation.

P_total - 0.581P_total = 0.737 atm

0.419P_total = 0.737 atm

P_total = 0.737 atm/0.419

P_total = 1.76 atm

Using P_total , calculate Partial pressure of fluorine,P_F2

P_F2 = mole fraction F₂ x P_total

P_F2 = 0.581 x 1.76 atm

P_F2 = 1.02 atm