Respuesta :
Answer:
11.3 g of [tex]NH_{3}[/tex] are produced from 36.0 g of [tex]H_{2}O[/tex]
Explanation:
1. The balanced chemical equation is the following:
[tex]Mg_{3}N_{2}(s)+6H_{2}O(l)=3Mg(OH)_{2}(s)+2NH_{3}(g)[/tex]
2. Use the molar mass of the [tex]H_{2}O[/tex], the molar mass of the [tex]NH_{3}[/tex] and the stoichiometry of the balanced chemical reaction to find how many grams of [tex]NH_{3}[/tex] are produced:
Molar mass [tex]H_{2}O[/tex] = 18[tex]\frac{g}{mol}[/tex]
Molar mass [tex]NH_{3}[/tex] = 17[tex]\frac{g}{mol}[/tex]
[tex]36.0gH_{2}O*\frac{1molH_{2}O}{18gH_{2}O}*\frac{2molesNH_{3}}{6molesH_{2}O}*\frac{17gNH_{3}}{1molNH_{3}}=11.3gNH_{3}[/tex]
Therefore 11.3 g of [tex]NH_{3}[/tex] are produced from 36.0 g of [tex]H_{2}O[/tex]
The mass of NH₃ produced is 11.3 g. The correct option is the fourth option 11.3 g
The given chemical equation for the reaction is
Mg₃N₂(s) + 6H₂O(l) → 3Mg(OH)₂(s) + 2NH₃(g)
This means,
1 mole of Mg₃N₂ reacts with 6 moles of H₂O to produce 3 moles of Mg(OH)₂ and 2 moles of NH₃
To determine the mass of NH₃ produced,
First, we will determine the number of moles of H₂O that reacted
From the question
Mass of H₂O that reacted = 36.0 g
From the formula
[tex]Number\ of\ moles = \frac{Mass }{Molar\ mass}[/tex]
Molar mass of mass of H₂O = 18.0 g/mol
∴ [tex]Number\ of\ moles = \frac{36.0 }{18.0}[/tex]
[tex]Number\ of\ moles = 2.0 \ moles[/tex]
∴ Number of moles of H₂O that reacted = 2.0 moles
Now, from the balanced chemical equation,
6 moles of H₂O yields 2 moles of NH₃
∴ 2 moles of H₂O will yield [tex]\frac{2\times 2}{6}[/tex] moles of NH₃
[tex]\frac{2\times 2}{6}=\frac{2}{3}[/tex]
∴ [tex]\frac{2}{3} \ moles[/tex] of NH₃ is produced
Now, to determine the mass of NH₃ produced
From the formula
Mass = Number of moles × Molar mass
Number of moles of NH₃ = [tex]\frac{2}{3} \ moles[/tex]
Molar mass of NH₃ = 17.0 g/mol
∴ Mass of NH₃ produced = [tex]\frac{2}{3} \times 17.0[/tex]
Mass of NH₃ produced = [tex]\frac{34}{3}[/tex]
Mass of NH₃ produced = 11.3 g
Hence, the mass of NH₃ produced is 11.3 g. The correct option is the fourth option 11.3 g
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