1. The mass of hydrogen needed to react with 50 g of nitrogen is 10.71 g
2. the number of mole of hydrogen needed to react with 2 moles of nitrogen is
3. The volume of hydrogen needed to react with 5 L of nitrogen at STP is 15 L
N₂ + 3H₂ —> 2NH₃
Molar mass of N₂ = 14 × 2 = 28 g/mol
Mass of N₂ from the balanced equation = 1 × 28 = 28 g
Molar mass of H₂ = 2 × 1 = 2 g/mol
Mass of H₂ from the balanced equation = 3 × 2 = 6 g
SUMMARY
From the balanced equation above,
28 g of N₂ reacted with 6 g of H₂
From the balanced equation above,
28 g of N₂ reacted with 6 g of H₂
Therefore,
50 g of N₂ will react with = (50 × 6) / 28 = 10.71 g of H₂
Balanced equation
N₂ + 3H₂ —> 2NH₃
From the balanced equation above,
1 mole of N₂ reacted with 3 moles of H₂
Therefore,
2 moles of N₂ will react with = 2 × 3 = 6 moles of H₂
Balanced equation
N₂(g) + 3H₂(g) —> 2NH₃(g)
At standard temperature and pressure (STP) and considering the balanced equation,
1 L of N₂ reacted with 3 L of H₂
Therefore,
5 L of N₂ will react with = 5 × 3 = 15 L of H₂
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