Percentage Yield
- Often in a chemical reaction, the amount of a product recovered is less than might have been expected from the amounts of the reactants used
Reasons for this include;
- The reaction may not have gone to completion because it is slow or reversible
- There may be competing side reactions which convert a proportion of the reactants into different products
- Some product may have been lost during purification
% Yield = actual moles of product/theoretical moles of product x 100
Atom economy
- A reaction may be intrinsically wasteful of there is more than one product and they are not all useful
Atom economy = Mr of desired product/sum of desired Mr of all products x 100
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