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

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

Step-by-step 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)*(1molMg(OH)_(2))/(58.3gMg(OH)_(2))*(6molesH_(2)O)/(3molesMg(OH)_(2))*(18gH_(2)O)/(1molH_(2)O)=93gH_(2)O`