1.1.17

Percentage Yield

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Percentage Yield

The percentage yield for any reaction is usually less than 100%. The following 5 factors cause deviations from 100%.

Incomplete reactions

Incomplete reactions

  • An incomplete reaction can happen because:
    • The reaction is very slow and hasn't been given enough time to happen.
  • The reaction is reversible and some of the products have turned back into reactants.
  • This reduces the percentage yield.
Waste

Waste

  • Some of the chemicals will remain stuck to the glassware and will be wasted.
  • This reduces the percentage yield.
Extraction

Extraction

  • It might be difficult to fully separate the product from the reaction mixture.
  • This reduces the percentage yield.
Side reactions

Side reactions

  • Unexpected reactions (side reactions) can happen. This may mean that the intended product is not created.
  • This reduces the percentage yield.
Hydration

Hydration

  • If a reaction is carried out in water, any extracted product may be 'wet'
  • This means that there is water in the extracted product.
    • Water is generally extremely difficult to fully remove from a product.
  • If a percentage yield is calculated to be over 100%, it is likely that your product is full of water.

Calculating Percentage Yield

The percentage yield of a reaction is calculated as the real yield divided by the theoretical yield multiplied by 100.

Real yield

Real yield

  • The real yield is the mass of the desired product obtained from a reaction.
Theoretical yield

Theoretical yield

  • The theoretical yield is the maximum mass of a product that could possibly be created from a reaction.
  • This can be calculated from a balanced equation if we know the mass of the reactants.
Percentage yield

Percentage yield

  • A comparison of the real and theoretical yields of a reaction.
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