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

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.