Nitrogen gas reacts with hydrogen gas to produce ammonia via the following reaction:

Question

N2 (g) + 3H2(g) →2NH3 (g)
How many grams of NH3 can be produced from 13.0 g of H2?
Express your answer with the appropriate units.

Answer 1

To find the number of grams of NH3 produced from 13.0 g of H2, we need to use stoichiometry.

From the balanced chemical equation, we can see that the mole ratio of H2 to NH3 is 3:2. This means that for every 3 moles of H2, 2 moles of NH3 are produced.

First, we need to determine the number of moles of H2 in 13.0 g of H2. To do this, we use the molar mass of H2.

Molar mass of H2 = 2.02 g/mol

Moles of H2 = (mass of H2) / (molar mass of H2)
= 13.0 g / 2.02 g/mol
= 6.44 mol

Now, using the mole ratio of H2 to NH3, we can determine the number of moles of NH3 produced.

Moles of NH3 = (moles of H2) * (2 moles NH3 / 3 moles H2)
= 6.44 mol * (2/3)
= 4.29 mol

Finally, we can find the mass of NH3 produced from the number of moles of NH3.

Molar mass of NH3 = 17.03 g/mol

Mass of NH3 = (moles of NH3) * (molar mass of NH3)
= 4.29 mol * 17.03 g/mol
= 73.01 g

Therefore, 13.0 g of H2 can produce 73.01 g of NH3.