What would cause the percent yield of a reaction to be less than 100%?

All of the limiting reagent gets used up.

The product participates in a side reaction.

Pure reactants are used.

A balanced chemical equation is used.

The reason why percentage yield for a chemical reaction can be less than a 100% is due to the presence of competing side reactions. As often the case and basics for all chemical reactions, mass and matter must be conserved. But sometimes the yield can be lower due to other reactions that must be considered.

A competing side reaction that can affect the yield of products during a chemical procedure is often one in which some of the products can react with some molecules present in the environment or some of the unused reactants when available.
Sometimes, a product can be hygroscopic, deliquescent or probably effervescent. This will definitely alter the expected amount of product one desires in a reaction based on stoichiometry.

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What would cause the percent yield of a reaction to be less than 100%? All of the limiting reagent gets used up. The product participates in a side reaction. Pure reactants are used. A balanced chemical equation is used.

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What would cause the percent yield of a reaction to be less than 100%?

All of the limiting reagent gets used up.

The product participates in a side reaction.

Pure reactants are used.

A balanced chemical equation is used.