Question

In the balanced reaction: 2Mg3N2(s)+3O2 --> 6MgO(s)+2N2

In a reaction, 18.05 moles of nitrogen were formed. How many moles of magnesium oxide were also formed?

Also, How many grams of Oxygen are needed to react with 3.277g of Mg3N2?

Answer 1

Answer:

From the reaction,

2 moles of N2 is formed from 2 moles Mg3N2

Let 18.05 moles be formed from x moles of Mg3N2.

Then x = 18.05 moles Mg3N2

Moles of magnesium oxide formed,

18.05 moles Mg3N2 * 6moles MgO / 2 moles Mg3N2

= 18.05 * 6 / 2

= 54.15 moles of MgO

Grams of O2 required to react with 3.227 g of Mg3N2,

Molar mass of Mg3N2 = 101g

No of moles of 3.227g of it = 3.227 / 101

= 0.031 moles of Mg3N2

Grams of oxygen required to react with 0.031 moles of Mg3N2,

= 0.031 moles Mg3N2 * 3 moles O2 * 32g / 2 moles Mg3N2

= 0.031 * 3 * 32 / 2 (molar mass of O2= 32g)

= 1.48 g of O2