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N2 + 3H2 = 2NH3
1) How many grams of hydrogen are necessary to react completely with 50 grams of nitrogen in the above equation? Please show work.
2) How many moles of hydrogen are needed to completely react with two moles of nitrogen? Please show work.
3) What volume of hydrogen in above reaction is necessary to react with five L of nitrogen to produce ammonia at STP? Please show work.

Sagot :

Eduard22sly

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

Balanced equation

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

1. How to determine the mass of hydrogen needed to react with 50 g of nitrogen

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

2. How to determine moles of hydrogen needed to react with 2 moles of nitrogen

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

3. How to determine the volume of hydrogen needed to react with 5 L of nitrogen

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

Learn more about stoichiometry:

https://brainly.com/question/14735801

https://brainly.com/question/13705779

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