Given the balanced equation: 3 H2 + N2 🡪 2 NH3 , how many moles of NH3 will be produced if 50.8 g N2 reacts with 187.3 g H2?

Question

Given the balanced equation: 3 H2 + N2 🡪 2 NH3 ,  

how many moles of NH3 will be produced if 50.8 g N2 reacts with 187.3 g H2? 

Answer 1

3H₂ + N₂ ==> 2NH₃ ... balanced equation

Find limiting reactant. An easy way is to divide mols of each reactant by the corresponding coefficient in the balance equation and whichever value is less indicates the limiting reactant.

H₂: 187.3 g x 1 mol H2 / 2 g = 93.65 mols H2 (÷3->31.2)

N₂: 50.8 g x 1 mol N2 / 28 g = 25.4 mols N2 (÷1->25.4)

Since 25.4 is less than 31.2, N₂ is limiting

Use moles limiting reactant to find mols of product that can be formed

25.4 mols N₂ x 2 mols NH₃ / mol N₂ = 50.8 mols NH₃ that can form