Question

For the question(s) that follow, consider the following balanced equation. Mg3N2(s) + 6H2O(l) → 3Mg(OH)2(s) + 2NH3(g) How many grams of H2O are needed to produce 150 g of Mg(OH)2? For the question(s) that follow, consider the following balanced equation. Mg3N2(s) + 6H2O(l) → 3Mg(OH)2(s) + 2NH3(g) How many grams of H2O are needed to produce 150 g of Mg(OH)2? 93 g 46 g 23 g 130 g 18 g

Answer 1

Answer:

93 g of $H_{2}O$ are needed to produce 150 g of $Mg(OH)_{2}$

Explanation:

1. Writhe the balanced equation given by the problem:

$Mg_{3}N_{2}(s)+6H_{2}O(l)=3Mg(OH)_{2}(s)+2NH_{3}(g)$

2. Then use the stoichiometry of the reaction to calculate the mass of $H_{2}O$ that is needed to produce 150g of $Mg(OH)_{2}$:

It is important to take in account the molar mass of the $Mg(OH)_{2}$  and the $H_{2}O$ for the calculations.

Molar mass of the $Mg(OH)_{2}$ = 58.3g

Molar mass of the $H_{2}O$ = 18g

$150gMg(OH)_{2}*\frac{1molMg(OH)_{2}}{58.3gMg(OH)_{2}}*\frac{6molesH_{2}O}{3molesMg(OH)_{2}}*\frac{18gH_{2}O}{1molH_{2}O}=93gH_{2}O$