Yield - The amount of product made in a chemical reaction.

There are three types:

• Actual yield- what you get in the lab when the chemicals are mixed
• Theoretical yield- what the balanced equation tells you should make.
• Percent yield = Actual x 100 Theoretical

Details

• Percent yield tells us how “efficient” a reaction is.
• Percent yield can not be bigger than 100 %.

According to the following equation, 2H₂ + O₂ → 2H₂O, 143 grams of H₂O is expected to be produced. What is the % yield of H₂O if 138 g H₂O is produced from 16 g H₂ and excess O₂?

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According to the following reaction, N2 + 3H2 → 2NH3, 227 grams of NH3 is expected to be produced. What is the % yield of NH3 if 40.5 g NH3 is produced from 20.0 mole H2 and excess N2?

If, in the reaction below, 93 grams of Cl₂ produces 42 grams of CCl₄ what is the % yield?

 CS₂ + 3Cl₂ 🡺 CCl₄ + S₂Cl₂

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If, in the reaction below, 11 grams of Fe₃O₄ produces a 88.2% yield of Fe. How many grams are produced?

 Fe₃O₄ + 4H₂ 🡺 3Fe + 4H₂O

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