Question

Given the equation: n2 202--> 2noz, what mass of oxygen is required to react completely with 71.909 g of nitrogen?

Answer 1

To determine the mass of oxygen required to react completely with nitrogen, we need to start by balancing the equation.

The balanced equation for the reaction is:
2N₂ + O₂ → 2N₂O

From the balanced equation, we can see that 2 moles of nitrogen react with 1 mole of oxygen to produce 2 moles of nitrogen oxide.

To calculate the mass of oxygen required, we'll use the molar masses of nitrogen (N₂) and oxygen (O₂) as well as the given mass of nitrogen (71.909 g).

The molar mass of nitrogen (N₂) is 28.02 g/mol.
The molar mass of oxygen (O₂) is 32.00 g/mol.

First, we need to calculate the number of moles of nitrogen:
moles of nitrogen = mass of nitrogen / molar mass of nitrogen
= 71.909 g / 28.02 g/mol
≈ 2.566 mol

Since 2 moles of nitrogen react with 1 mole of oxygen, we can calculate the moles of oxygen required:
moles of oxygen = (2/1) * moles of nitrogen
= 2.566 mol
≈ 5.132 mol

Finally, we can calculate the mass of oxygen required:
mass of oxygen = moles of oxygen * molar mass of oxygen
= 5.132 mol * 32.00 g/mol
≈ 164.224 g

Therefore, approximately 164.224 g of oxygen is required to react completely with 71.909 g of nitrogen.