# Chapter 9 - Stoichiometry

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Composition Stoichiometry
calculations involving the mass relationships of elements in compounds
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Reaction Stoichiometry
calculations involving the mass relationships between reactants and products in a chemical reaction
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Mole Ratio
a conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction
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Stoichiometry
(chemistry) the relation between the quantities of substances that take part in a reaction or form a compound (typically a ratio of whole integers)
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Limiting Reactant
the reactant that limits the amounts of the other reactants that can combine and the amount of product that can form in a chemical reaction
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Excess Reactant
the substance that is not used up completely in a reaction
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Percentage Yield
the ratio of the actual yield to the theoretical yield multiplied by 100
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Actual Yield
the amount of product that actually forms when the reaction is carried out in the laboratory
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Theoretical Yield
the amount of product that could form during a reaction calculated from a balanced chemical equation; it represents the maximum amount of product that could be formed from a given amount of reactant
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Given the Balanced Reaction: 2Al2O3(l) ā 4Al(s) + 3O2(g) How many moles of O2 will be formed if 10 moles of Al2O3 are used?
15 moles of O2
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Given the reaction: NH3(g) + O2(g) ā NO(g) + H2O(g) What is the limiting reactant when there are .5 moles of O2 and 1.5 moles of NH3 available to react? How much excess is there?
O2, there is .1 moles of excess NH3.
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If you have an actual yield of 72.3 g of product and the theoreticla yield is 78.7 g, what is your % yield?