Review Session Exam 2 - Review Session Exam 2 Calculations...

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Review Session Exam 2 Calculations with Moles Through End of Chapter 4 (plus anything needed from Exam 1)
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Exam Topics The mole Know how to calculate moles Number of atoms, ions, and molecules in a mole Know the definition Formula Weights, molecular weights and moles Calculate the molar mass of a compound
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Example Question 1 E-1 How many moles of K 2 HPO 4 are there in 22.8 g of potassium hydrogen phosphate?
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Example Question 2 E-2 How many moles of oxygen atoms are there in 22.8 g of potassium hydrogen phosphate?
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Exam Topics Percent Composition and Formulas of Compounds Derivation of Formulas from Elemental Composition mass of element Percent Composition of element = 100% mass of compound e
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Example Question 3 E-3. In an experiment, 6.2g of phosphorus combined with oxygen to form 14.2g of phosphorus oxide. Calculate the empirical formula of the oxide. (If the answer were C 3 H 8 , type it in as C3H8)
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Exam Topics Other interpretations of Chemical Formulas Know how to calculate mass of an element from the mass of a formula Know how to calculate mass of a compound from a given mass of an element Percent Purity Percentage of the pure compound in the whole sample
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Exam Topics Chemical Equations Know how to balance chemical equations Understand mole ratios Calculations based on Chemical Equations Must work with moles, formula units, atoms, ions, or molecules Masses (g, kg, lb, tons, etc.) must be converted to moles
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Example Question 4 Balance the following equation for the combustion of allene with oxygen: C 3 H 4 + O 2 CO 2 + H 2 O Express the answer as a series of numbers, for example 6149 for 6 allenes, 1 oxygen, 4 carbon dioxides, and 9 waters. If there is only 1 for a component, put in the 1.
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Exam Topics The Limiting Reactant Concept Remember: Reagent is the same as Reactant Must find which reactant produces the least product. Any product from the reaction can be used. The reactant the produces the least product is the limiting reactant.
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Example Question 5 Which is the limiting reactant in the following reaction? Na 2 CO 3(aq) + 2AgNO 3(aq) Ag 2 CO 3(s) + NaNO 3(aq) 2.33g 8.67 g A. Na 2 CO 3(aq) A. AgNO 3(aq)
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Example Question 6 How much silver carbonate is produced in the following reaction in the following reaction? Na 2 CO 3(aq) + 2AgNO 3(aq) Ag 2 CO 3(s) + NaNO 3(aq) 2.33g 8.67 g
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Exam Topics Percent Yields from Chemical Reactions The theoretical yield is the most that can be produced. This is determined by the limiting reactant. The actual yield is what is really produced by the experiment. It is less than or equal to the theoretical yield. Actual Yield Percent Yield = 100% Theoretical Yield e
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Exam Topics Percent Yields from Chemical Reactions Know how to calculate the percent yield from a limiting reactant and the actual yield Know how to calculate the theoretical yield from the percent yield and the actual yield Know how to calculate the actual yield from a limiting reactant and the percent yield
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This note was uploaded on 08/26/2008 for the course CHEM 1211 taught by Professor Atwood during the Spring '07 term at University of Georgia Athens.

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Review Session Exam 2 - Review Session Exam 2 Calculations...

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