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Ch3 notes part 2 answers

Ch3 notes part 2 answers - Answers to sample Qs for CH3...

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Answers to sample Qs for CH3: part 2 Example 1 for Limiting Reagents: 4Fe + 3O 2 2Fe 2 O 3 I have 1 mole of oxygen gas and 2 moles of iron available. How much iron(III) oxide could be formed? How much iron or oxygen would be left unreacted? 1 moles O 2 x 2 moles Fe 2 O 3 = 0.66 moles Fe 2 O 3 3 moles O 2 2 moles Fe x 2 moles Fe 2 O 3 = 1 mole Fe 2 O 3 4 moles Fe 1 moles O 2 x 4 moles Fe = 1.3 moles Fe so we would have 0.66 moles Fe left over 3 moles O 2 Example 2 for Limiting Reagents: What is the maximum mass of sulfur dioxide that can be produced by the reaction of 95.6 g of carbon disulfide with 110. g of oxygen? CS 2 + 3O 2 CO 2 + 2SO 2 2 2 2 2 2 2 2 2 2 2 2 2 2 2 2 2 2 SO g 147 SO mol 1 SO g 1 . 64 O mol 3 SO mol 2 O g 32.0 O mol 1 O g 110 SO mol ? SO g 161 SO mol 1 SO g 1 . 64 CS mol 1 SO mol 2 g 76.2 CS mol 1 CS g 6 . 95 SO mol ? = × × × = = × × × = % 5 . 77 % 100 H COOC CH g 19.1 H COOC CH g 14.8 = yield % reaction. for the yield percent the Calculate . 2 H COOC CH g 1 . 19 H COOC CH mole 1 H COOC CH 88.0g OH H C mole 1 H COOC CH mole 1 OH H C g 0 . 46 OH H C
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