A magnesium ribbon, when burnt in air, left an ash containing MgO and Mg3N2. The ash was found to consume 0.6 mole of HCl, when it was taken in solution, according to the following reaction:Mg3N2 + 8HCl → 3MgCl2 + 2NH4ClThe solution obtained was treated with excess of NaOH, when 0.1 mole of NH3 was evolved. The mass (in g) of magnesium burnt is: 6

A magnesium ribbon, when burnt in air, left an ash containing MgO and

1.	A magnesium ribbon, when burnt in air, left an ash containing MgO and Mg3N2. The ash was found to consume 0.6 mole of HCl, when it was taken in solution, according to the following reaction:Mg3N2 + 8HCl → 3MgCl2 + 2NH4ClThe solution obtained was treated with excess of NaOH, when 0.1 mole of NH3 was evolved. The mass (in g) of magnesium burnt is: 6
Answer» A magnesium ribbon, when burnt in air, left an ash containing $M g O$ and $M g_{3} N_{2}$ . The ash was found to consume 0.6 mole of HCl, when it was taken in solution, according to the following reaction: $M g_{3} N_{2}$ + $8 H C l$ $\to$ $3 M g C l_{2}$ + $2 N H_{4} C l$ The solution obtained was treated with excess of $N a O H$ , when $0.1 m o l e$ of $N H_{3}$ was evolved. The mass (in $g$ ) of magnesium burnt is: 6