1. The mass of silane gas, SiH₄ formed from the reaction is 3.57 g
2. The mass of H₂O produced from the reaction is 173.75 g
<h3>1. How to determine the mass of SiH₄ formed</h3>
Balanced equation
Mg₂Si (s) + 4H₂O (l) ---> 2Mg(OH)₂ (aq) + SiH₄ (g)
Molar mass of Mg₂Si = (24×2) + 28 = 76 g/mol
Mass of Mg₂Si from the balanced equation = 1 × 76 = 76 g
Molar mass of SiH₄ = 28 + (4×1) = 32 g/mol
Mass of SiH₄ from the balanced equation = 1 × 32 = 32 g
SUMMARY
From the balanced equation above,
76 g of Mg₂Si reacted to produce 32 g of SiH₄
From the above information, we can obtain the mass of SiH₄ produced by the reaction of 8.48 g of Mg₂Si as illustrated below:
From the balanced equation above,
76 g of Mg₂Si reacted to produce 32 g of SiH₄
Therefore,
8.48 g of Mg₂Si will react to produce = (8.48 × 32) / 76 = 3.57 g of SiH₄
Thus, 3.57 g of SiH₄ were obtained from the reaction.
<h3>2. how to determine the mass of H₂O produced</h3>
Balanced equation
4NH₃ (g) + 7O₂ (g) ---> 4NO₂ (g) + 6H₂O (g)
Molar mass of NH₃ = 14 + (1×3) = 17 g/mol
Mass of NH₄ from the balanced equation = 4 × 17 = 68 g
Molar mass of H₂O = (2×1) + 16 = 18 g/mol
Mass of H₂O from the balanced equation = 6 × 18 = 108 g
SUMMARY
From the balanced equation above,
68 g of NH₃ reacted to produce 108 g of H₂O
From the above information, we can obtain the mass of H₂O produced by the reaction of 109.4 g of NH₃ as illustrated below:
From the balanced equation above,
68 g of NH₃reacted to produce 108 g of H₂O
Therefore,
109.4 g of NH₃ will react to produce = (109.4 × 108) / 68 = 173.75 g of H₂O
Thus, 173.75 g of H₂O were obtained from the reaction.
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