Question

If 7.45g of N2 and 36.5mL of 0.150M O2 react together, how many grams of N2O gas will be produced?

Answer 1

Answer:

0.482 g of N₂O are produced.

Explanation:

The reaction is: 2N₂ + O₂ →  2N₂O

In order to produce 2 moles of N₂O, we need to make react 1 mol of oxygen and 2 moles of nitrogen.

We determine the moles of each reactant:

7.45 g / 28g/mol = 0.266 moles of nitrogen

36.5 mL . 0.15 M = 5.475 mmoles →  . 1mol /1000 mmol = 0.00547 moles

Certainly the oxygen is the limiting reactant.

In order to determine the grams produced, we need to know the limiting reactant.

2 moles of N₂ need 1 mol of O₂

Then 0.266 moles of N₂ may react to (0.266 . 1) /2 = 0.133 moles

We only have 0.00547 moles, so there is not enough O₂.

1 mol of O₂ can produce 2 moles of N₂O

Then, the 0.00547 will produce (0.00547 . 2) /1 = 0.01095 moles

We convert to mass: 0.01095 mol . 44 g /mol = 0.482 g

That's the answer.