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NIS – CHEMISTRY. Lecture 65 Percent Yield Ozgur Unal. Percent Yield. Some popcorns remain unpopped.... Similarly, in a chemical reaction, not all the reactants react to produce a product. There can be several reasons for this:

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NIS – CHEMISTRY

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NIS – CHEMISTRY

Lecture 65

Percent Yield

OzgurUnal


Percent Yield

  • Some popcorns remain unpopped....

  • Similarly, in a chemical reaction, not all the reactants react to produce a product.

  • There can be several reasons for this:

    • Liquid reactants might adhere to the surfaces of their containers or evaporate.

    • Products other than intended ones might be formed bu competing reactions

  • These factors reduce the yield of the desired product.

When you pop a bag of popcorn, do all of the popcorns pop inside the bag?


Percent Yield

  • Chemists need to know how efficient a reaction is in producing the desired product.

  • One way of measuring efficiency is by means of percent yield.

  • Percent yield of product is the ratio of the actual yield to the theoretical yield expressed as a percent

  • percent yield = 100 * actual yield / theoretical yield

In our previous calculations, we determined the amounts of the products formed in chemical reactions  Theoretical yield

A reaction rarely produces the theoretical yield of product.

The actual yield is the amount of product produced when the chemical reaction is carried out in an experiment.


Percent Yield

Example: Solid silver chromate (Ag2CrO4) forms when potassium chromate (K2CrO4) is added to a solution containing 0.500 g of silver nitrate. Determine the theoretical yield of Ag2CrO4. Calculate the percent yield if the reaction yields 0.455 g of Ag2CrO4.

  • Example:Zinc reacts with iodine in a synthesis reaction. Determine the theoretical yield if 1.912 mol of zinc is used.Determine the percent yield if 515.6 g of product is recovered.


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