Actual Yield Definition . The actual yield is the quantity of a product that is obtained from a chemical reaction.In contrast, the calculated or theoretical yield is the amount of product that could be obtained from a reaction if all of the reactant converted to product. Theoretical yield is based on the limiting reactant.
Of course, a “true” actual yield can NEVER be greater than the “true” theoretical yield in a reaction ( this is the answer to the last question you posed ). What I mean by a “true” theoretical yield is the theoretical yield wherein you have accounted ALL of the possible occurrences in your reaction.
Use the molar mass of the product to convert moles product to grams of product. In equation form: grams product = grams reactant x (1 mol reactant/molar mass of reactant) x (mole ratio product/reactant) x (molar mass of product/1 mol product) The theoretical yield of our reaction is calculated using: molar mass of H 2 gas = 2 grams.
Percent yield represents the ratio between what is experimentally obtained and what is theoretically calculated, multiplied by 100%. #"% yield" = ("actual yield")/("theoretical yield") * 100%# So, let's say you want to do an experiment in the lab. You want to measure how much water is produced when 12.0 g of glucose (#C_6H_12O_6#) is burned with enough oxygen.
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