Percent Yield Theoretical Yield Actual Yield

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Presentation transcript:

Percent Yield Theoretical Yield Actual Yield

Theoretical Yield The maximum amount of product that can be formed from given amounts of reactants The amount you should get in a perfect world Use equation and stoichiometry to calculate this amount

Actual Yield The amount of product that actually forms when a reaction is carried out in the lab

A measure of the efficiency of a reaction carried out in the lab Percent Yield A measure of the efficiency of a reaction carried out in the lab The ratio of the actual yield to the theoretical yield Percent yield = actual yield x 100% theoretical yield

Percent yield should not be greater than 100% Often less than 100% Rxns. don’t always go to completion Some product can be lost during filtering or transferring Reactants or products not measured carefully

When 84.8 g of iron(III) oxide reacts with an excess of carbon monoxide, iron is produced. Fe2O3(s) + 3CO(g)  2Fe(s) + 3CO2(g) What is the theoretical yield of iron?

In an experiment, 50.0 g of silicon dioxide is heated with an excess of carbon, and 27.9 g of silicon carbide is produced. SiO2(g) + 3C(s)  SiC(s) + 2CO(g) What is the percent yield of this reaction?

When 5.00 g of copper reacts with excess silver nitrate, silver metal and copper(II) nitrate are produced. What is the theoretical yield of silver in this reaction?