The reaction N2 + 3 H2 → 2 NH3 is used to produce ammonia. When 450. g of hydrogen was reacted with nitrogen, 1575 g of ammonia were produced. What is the percent yield of this reaction?

The percent yield of this reaction is 70%

Explanation:

The reaction is: N₂ + 3H₂ → 2NH₃

We only have the mass of H₂, so we assume that N₂ is in excess

We convert the mass to moles, to work with the reaction:

450 g. 1mol / 2 g = 225 moles

Ratio is 2:3. 3 moles of H₂ can produce 2 moles of ammonia

Therefore 225 moles of H₂ will produce (225.2) / 3 = 150 moles

This is the 100% yield reaction → We convert the moles of NH₃ to mass

150 mol. 17g / 1mol = 2550 g

Percent yield = (Produced yield/Theoretical yield).100

Percent yield = (1575g/2550g). 100 = 70%