What is the partial pressure of N2 if the total pressure of a container with both nitrogen and carbon dioxide gas 1.604 atm and carbon dioxides partial pressure is 41.80 kPa?

Partial pressure N₂ = 1.191 atm

Explanation:

This is an easy problem to solve

In a mixture of gases, when we sum the partial pressure of each gas we obtained the total pressure of the mixture.

Partial pressure N₂ + Partial pressure CO₂ = Total pressure

Partial pressure N₂ + 41.80 kPa = 1.604 atm

Let's convert the partial pressure of CO₂ from kPa to atm, in order to have the same units → 41.80 kPa. 1atm / 101.3 kPa = 0.413 atm

Partial pressure N₂ = 1.604 atm - 0.413 atm → 1.191 atm

The partial pressure of N2 is 1.1914661 atm

Explanation:

Step 1: Data given

Total pressure = 1.604 atm

Partial pressure of CO2 = 41.80 kPa = 0.4125339 atm

Step 2: Convert kPa to atmosphere

41.80 / 101.325 = 0.4125339 atm

Step 3: Calculate partial pressure of N2

Total pressure = partial pressure N2 + partial pressure CO2

Partial pressure N2 = total pressure - partial pressure CO2

Partial pressure N2 = 1.604 atm - 0.4125339

Partial pressure N2 = 1.1914661 atm

The partial pressure of N2 is 1.1914661 atm