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Kay [80]
4 years ago
6

For the question(s) that follow, consider the following balanced equation. Mg3N2(s) + 6H2O(l) → 3Mg(OH)2(s) + 2NH3(g) How many g

rams 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
Chemistry
1 answer:
Slav-nsk [51]4 years ago
6 0

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

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