Answer:
0.0554 moles of Mg3N2 are needed.
Explanation:
1st) From the given balanced quation we know that 1 mole of Mg3N2 reacts with 6 moles of H2O to produce 3 moles of Mg(OH)2 and 2 moles of NH3.
2nd) With the molar mass of Mg(OH)2 (58.32g/mol) we can convert moles to grams:
[tex]3mol*\frac{58.32g}{1mol}=174.96g[/tex]Now we know that 1 mole of Mg3N2 produces 174.96g of Mg(OH)2.
3rd) From the balanced equation we know that 174.96g of Mg(OH)2 are produced from 1 mole of Mg3N2, so to produce 9.69 grams of Mg(OH)2 we can use a mathematical rule of three to calculate the moles of Mg3N2 needed:
[tex]\begin{gathered} 174.96g\text{ Mg\lparen OH\rparen}_2-1mole\text{ Mg}_3\text{ N}_2 \\ 9.69g\text{ Mg\lparen OH\rparen}_2-x=\frac{9.69g\text{ Mg\lparen OH\rparen}_2*1mole\text{ Mg}_3\text{ N}_2}{174.96g\text{ Mg\lparen OH\rparen}_2} \\ x=0.0554moles\text{ Mg}_3\text{ N}_2 \\ \end{gathered}[/tex]Finally, 0.0554 moles of Mg3N2 are needed.
