If 56 grams of nitrogen is mixed with 56 grams of oxygen, what is the pressure of each gas if the total pressure is 1320 Torrs?

pN₂ = 695 torr; pO₂ = 625 torr

Explanation:

Step 1: Calculate the moles of each gas

The molar mass of N₂ is 28.01 g/mol.

56 g × 1 mol/28.01 g = 2.0 mol

The molar mass of O₂ is 32.00 g/mol.

56 g × 1 mol/32.00 g = 1.8 mol

Step 2: Calculate the total number of moles

n = nO₂ + nN₂ = 1.8 mol + 2.0 mol = 3.8 mol

Step 3: Calculate the partial pressure of each gas

We will use the following expressions.

pN₂ = P × X(N₂)

pN₂ = 1320 torr × (2.0 mol/3.8 mol)

pN₂ = 695 torr

pO₂ = P × X(O₂)

pO₂ = 1320 torr × (1.8 mol/3.8 mol)

pO₂ = 625 torr

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)