1. Percent Yield

2. Yield u The amount of product made in a chemical reaction. u There are three types u Actual yield- what you get in the lab when the chemicals are mixed u Theoretical yield- what the balanced equation tells you you should make. u Percent yield u Percent yield = Actual x 100 % Theoretical

3. Example u 6.78 g of copper is produced when 3.92 g of Al are reacted with excess copper (II) sulfate.  2Al + 3 CuSO 4  Al 2 (SO 4 ) 3 + 3Cu u What is the actual yield? u What is the theoretical yield? u What is the percent yield?

4. Details u Percent yield tells us how “efficient” a reaction is. u Percent yield can not be bigger than 100 %.

5. Example u Methanol (CH 3 OH) is the simplest alcohol. It is used as a fuel in race cars and is a potential replacement for gasoline. Methanol can be manufactured by combining gaseous carbon monoxide and hydrogen. Suppose 68.5kg of CO is reacted with 8.60kg H 2. Calculate the theoretical yield of methanol. If 3.57 x 10 4 g of methanol is actually produced, what is the percent yield of methanol?