Chapter 12 Stoichiometry – Flashcards
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| How is a balanced equation like a recipe? |
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| a balanced chemical equation provides the same kind of quantitative information that a recipe does. |
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| How does a chemist use balanced chemical equation? |
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| chemists use balanced chemical equations as a basis to calculate how much reactant is needed or product is formed in a reaction. |
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| In terms of what quantities can you interpret a balanced chemical equation? |
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| a balanced chemical equation can be interpreted in terms of different quantities, including numbers of atoms, molecules, or moles; mass; and volume. |
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| What quantities are conserved in every chemical reaction? |
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| mass and atoms are conserved in every chemical reaction. |
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| Stoichiometry |
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| A subject of chemistry that focuses on the calculations of quantities in chemical reactions. |
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| How are mole ratios used in chemical calculations? |
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| in chemical calculations, mole ratios are used to convert between moles of reactant and moles of product, between moles of reactants, or between moles of products. |
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| What is the general procedure for solving a stoichiometric problem? |
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| in a typical stoichiometric problem, the given quantity is first converted to moles. Then the mole ratio from the balanced equation is used to calculate the number of moles of the wanted substance. Finally, the moles are converted to any other unit of measurement related to the unti mole, as the problem requires. |
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| Mole ratio |
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| a conversion factor derived from the coeffiecients of a balanced chemical equation interpreted in terms of moles. |
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| How is the amount of product in a reaction affected by an insufficient quantity of any of the reactants? |
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| in a chemical reaction, an insufficient quantity of any of the reactants will limit the amount of product that forms. |
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| What does the percent yield of a reaction measure? |
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| the percent yield is a measure of the efficiency of a reaction carried out in the laboratory. |
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| Limiting reagent |
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| the reagent that determines the amount of product that can be formed by a reaction. |
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| Excess reagent |
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| the reactant that is not completely used up in a reaction. |
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| Theoretical yield |
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| the maximum amount of product that could be formed from given amounts of reactants. |
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| Actual yield |
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| the amount of product that actually forms when the reaction is carried out. |
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| Percent yield |
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| the ratio of the actual yield to the theoretical yield expressed as a percent. |
