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### Percent Yield

### Percent Yield

### 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?

- 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.

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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