Question

The following reactions are carried out:

$A:$ Nitrogen + metal $\to$ compound $X$

$B:$ $X$ + water $\to$ ammonia + another compound

$C:$ Ammonia + metal oxide $\to$ metal + water + $N_2$

One metal that can be used for reaction $A$ is magnesium. Write the correctly balanced equation for reaction $B$, where $X$ is the compound formed.

• A. $Na{N}_2+H_{2}O\to {NH}_3+N{a}_{2}O$
• B. ${Mg}_3{N}_2+{3H}_{2}O\to {2NH}_3+3MgO$
• C. ${Ca}_3{N}_2+H_{2}O\to {NH}_3+CaO$
• D. None of these

Answer 1

The correct option is D None of these

One metal that can be used for reaction A is magnesium. So the corresponding reaction A is $N_2+3Mg\to M{g}_3{N}_2$

Hence the compound X is $-M{g}_3{N}_2$.

The complete reactions involving $Mg$ are as follows:

A: $N_2+3Mg\to M{g}_3{N}_2$

B: $M{g}_3{N}_2+6H_{2}O\to 3Mg(OH{)}_2+2N{H}_3$

C: $2N{H}_3+3MgO\to 3Mg+3H_{2}O+N_2$

The correct balanced equation for reaction B is $M{g}_3{N}_2+6H_{2}O\to 3Mg(OH{)}_2+2N{H}_3$