lect_11oct22f08

# lect_11oct22f08 - Outline 11 22-OCT-2008 1.ReviewQuestions...

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1 Outline 11 22-OCT-2008 1.Review- Questions? Stoichiometry needs Limiting reagent (Least amount, ratio, ICE) 2. % yield 3. Solution Concentrations, mol/L Another way to get moles! 4. Solution Stoichiometry

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2 Theoretical and Percent Yield Theoretical yield of product - maximum amount of product that can be obtained from given amounts of reactants. Percentage yield - actual yield (experiment) expressed as % of theoretical yield (calculated). % 100 yield l theoretica yield actual Yield % × =
3 Theoretical and Percent Yield Ex: (cont.) (calculation of % yield) recall that theoretical yield of H 2 in a previous example (lecture #10, slides 8 or 9 or 12. was 0.26 mol (or 0.52 g) H 2 . If actual yield of reaction had been 0.22 g H 2 , then % 42 % 100 H g 0.52 H g 0.22 Yield % 2 2 = × =

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4 Stoichiometry & % yield: Ex. 1 Prob: 3.76; 158 g aluminum sulfide (150. g/mol) and 131 g water (18.0 g/mol) are mixed making hydrosulfuric acid (34.0 g/mol) and aluminum hydroxide (78.0 g/mol). (a) Write balanced chem. eqn. (b) Calculate mol and grams hydrosulfuric acid that can be (c) How many grams excess reactant remain? (d) If only 75 g of H 2 S are obtained what is the % yield?
5 Prob: 3.76; 158 g aluminum sulfide and 131 g water are mixed making hydrosulfuric acid and aluminum hydroxide. (a) Write balanced chem. eqn. __ Al 2 S 3 + __ H 2 O __ Al(OH) 3 + __ H 2 S Al 2 S 3 + 6 H 2 O → 2 Al(OH) 3 + 3 H 2 S

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6 Prob: 3.76; 158 g aluminum sulfide and 131 g water are mixed making hydrosulfuric acid and aluminum hydroxide. Al
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## This note was uploaded on 02/18/2009 for the course CHEM 1A taught by Professor Okamura during the Fall '08 term at UC Riverside.

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lect_11oct22f08 - Outline 11 22-OCT-2008 1.ReviewQuestions...

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