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If the theoretical yield of a product is 345g but the actual yield is only 335g,...
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- 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.
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:
Posted by jerichorayel on April 25, 2013 at 2:42 AM (Answer #1)
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