If the theoretical yield of a product is 345g but the actual yield is only 335g, calculate the percent yield of the product. Explain at least 3 factors that may have resulted in the actual yield...

If the theoretical yield of a product is 345g but the actual yield is only 335g, calculate the percent yield of the product. Explain at least 3 factors that may have resulted in the actual yield not reaching the theoretical yield.

Asked on by danielb77

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jerichorayel | College Teacher | (Level 2) Senior Educator

Posted on

To get the percentage yield, we use the expression:

`% yield = (actual yield)/(theo retical yield) * 100`

To solve for the percent yield of the product,

`% yield = (335)/(345) * 100`

`% yield = 97.1 %`

Factors that affect the percent yield:

  • The reaction may be reversible; meaning, the product/s may form back the reactant at some point in time. We can also say that the reaction may not go into completion.
  • Some of the products may be left in the [walls of the] apparatus
  • Poor weighing, collection and transfer methods in the laboratory which may affect the amount of the products or reactants.
  • Reaction maybe too slow to be stoichiometric.
Sources:

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