# 8.3: Limiting Reagents and Percent Yield

```Standards and Checkpoints: Unit 8
8.1: Mole Ratios
Use mole ratios from balanced chemical equations.
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Given a balanced chemical equation (or enough information to write one), construct conversion factors that
relate moles of any two reactants or products in the reaction.
Given a balanced chemical equation (or enough information to write one), convert from moles of one reactant or
product to moles of any other reactant or product.
8.2: Mass-Mass Stoichiometry
Use mole ratios from balanced chemical equations in combination with mass -mole conversions.
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Given a balanced chemical equation (or enough information to write one), convert from mass of one reactant or
product to mass of any other reactant or product.
8.3: Limiting Reagents and Percent Yield
Use stoichiometry to identify limiting reagents, and calculate theoretical and percent yields.
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Given the masses of two or more reactants, identify the limiting reagent and calculate the theoretical yield
(the maximum mass of product that could form from the reaction between them.)
Given a description of a specific chemical reaction, explain why a chemist might decide to add one of the
reactants (rather than the others) in excess.
Describe why the actual yield in a chemical reaction is less than the theoretical yield.
Given an actual yield and a theoretical yield (or enough information to calculate a theoretical yield) for a chemical
reaction, calculate the percent yield for the reaction.
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