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Given the following reaction:1 NH4NO2 (s) = 1 N2 (g) + 2 H2O (g)How many liters of nitrogen gas is produced if 25.5 L of water is produced at STP?

User Irfan DANISH
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1 Answer

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Step-by-step explanation:

N₂ and H₂O are produced according to the following equation.

NH₄NO₂ (s) ---> N₂ (g) + 2 H₂O (g)

We know that 1 mol of a gas at STP (standard conditions of temperature and pressure) will ocuppy 22.4 L. We can use this relationship to find the number of moles present in 25.5 L of water vapor.

1 mol of H₂O = 22.4 L

moles of H₂O = 25.5 L * 1 mol/(22.4 L)

moles of H₂O = 1.14 mol

NH₄NO₂ (s) ---> N₂ (g) + 2 H₂O (g)

According to the coefficients of the reaction's equation when 2 moles of H₂O are produced, 1 mol of N₂ is also produced. Then the molar ratio between H₂O and N₂ is 2 to 1. We can use that ratio to find the number of moles of N₂ that are produced.

2 moles of H₂O : 1 mol of N₂

moles of N₂ = 1.14 moles of H₂O * 1 mol of N₂/(2 moles of H₂O)

moles of N₂ = 0.57 moles

And finally we can convert the moles of N₂ into liters.

volume of N₂ = 0.57 moles * 22.4 L/mol

volume of N₂ = 12.8 L

Answer: 12.8 L of nitrogen are produced.

User Cherouvim
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