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Theoretical yield
From Wikipedia, the free encyclopedia
In synthetic chemistry, theoretical yield is the calculated maximum quantity of product that could possibly be produced in a chemical reaction. The theoretical yield for a specific reaction depends on the quantity of starting materials, particularly the limiting reagent. The theoretical yield is typically calculated assuming that there is only one reaction involved, that all of the reactant is converted into product, and that all the product is isolated in pure form. An ideal synthesis would produce 100% of the theoretical yield, but few reactions approach this threshold. In practice, the theoretical yield serves as a standard to measure the effectiveness (practical yield) of a synthetic procedure. Depending on the inherent limitations of the reaction and experience level of the chemist, a practical yield of 40-50% is considered successful, 80% would be excellent and 90%+ would be exceptional.
Percent yields also determine in which way the chemist was incorrect. If the percent yield is over 100%, it is because too much reactants were used, and the actual yield is higher than the theoretical.
A difference between theoretical yield and actual yield is the terminology used. For example, when writing chemicals, they are called reactant. So the reactants in a reaction would be what goes in. But the actual physical chemicals which are used in the experiment are called reagents.
%yield=Actual(Practical) Yield/Theoretical Yield
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