Three atoms of magnesium combine with 2 atoms of nitrogen. What will be the weight of magnesium which combines with 1.86 g of nitrogen?

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Solution

Balanced equation:
3Mg + N2 → Mg3N2 Molar mass of Mg = 24 g
3 mol atoms of Mg
= 24 g x 3 = 72 g
Molar mass of N = 14 g
2 mol atoms of N
= 14 g x 2 = 28 g
28 g N2 combines with 72 g of Mg Therefore 1.86 g of nitrogen will combine = 72 g Mg/28 g N2 x 1.86 g N2 = 4.78 g Mg

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Three atoms of magnesium combine with 2 atoms of nitrogen. What will be the weight of magnesium which combines with 1.86 g of nitrogen?

Balanced equation: 3Mg + N2 → Mg3N2 Molar mass of Mg = 24 g 3 mol atoms of Mg = 24 g x 3 = 72 g Molar mass of N = 14 g 2 mol atoms of N = 14 g x 2 = 28 g 28 g N2 combines with 72 g of Mg Therefore 1.86 g of nitrogen will combine = 72 g Mg/28 g N2 x 1.86 g N2​ = 4.78 g Mg

Balanced equation:
3Mg + N2 → Mg3N2 Molar mass of Mg = 24 g
3 mol atoms of Mg
= 24 g x 3 = 72 g
Molar mass of N = 14 g
2 mol atoms of N
= 14 g x 2 = 28 g
28 g N2 combines with 72 g of Mg Therefore 1.86 g of nitrogen will combine = 72 g Mg/28 g N2 x 1.86 g N2 = 4.78 g Mg