Percent Yield & Limiting Reactants

Calculate the percent yield of a reaction that had a theoretical yield of 3.76 g and an actual yield of 1.45 g.

39%

If the actual yield of a reaction was 0.567 g, and the theoretical yield was 0.750 g, what was the percent yield of this reaction?

75.6%

What is the percent yield of sulfur dioxide if the burning of carbon disulfide produces 40.5 g of sulfur dioxide when the theoretical yield is 42 g?

96%

45.6 g of benzene (C6H6) react to form chlorobenzene (C6H5Cl). If the actual yield is 63.7 g of chlorobenzene, calculate the percent yield. C6H6 (l) + Cl2 (g) C6H5Cl (s) + HCl (g)

97%

Limiting Reactant

A limiting reactant is the reactant that is completely consumed in a chemical reaction. This reactant limits the amount of product that can be produced.

Actual Yield

Amount of product formed when reaction is completed (measured)

Excess Reactant

An excess reactant is the reactant that is NOT completely consumed in a chemical reaction. Some of this reactant(s) will be left over after the reaction is complete.

Theoretical Yield

The maximum amount of product that can be produced from a given amount of reactant (calculated)

Percent Yield

The ratio of the actual yield to the theoretical yield expressed as a percent

Percent Yield Formula

actual yield/theoretical yield x 100