#### Related to [[Stoichiometry and balancing]] --- ## Definition - **The theoretical yield** of a chemical reaction is the amount of **product** that would be formed under ideal conditions when *all* of the reactants are used. - **The actual yield** is the amount of product you where able to get *in the real world*, it **will always/should always be less than the theoretical yield.** --- ## Reasons for a lower yield - Not all reactants are consumed. - There may be side reactions occurring producing other products. - There may be a reverse reaction happening. - Loss of product during filtering/purification steps. --- ## Percent yield >[!quote] >![[percent yield.png]] --- #subpage