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Chapter 11 Review

Chapter 11 Review. Define the following: . Stoichiometry Mole ratio Excess reactant Limiting reactant Theoretical yield Actual yield Percent yield. Find the following molar masses:. O2 O AlPO 4 NaCl C 6 H 5 Cl CuO.

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Chapter 11 Review

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  1. Chapter 11 Review

  2. Define the following: • Stoichiometry • Mole ratio • Excess reactant • Limiting reactant • Theoretical yield • Actual yield • Percent yield

  3. Find the following molar masses: • O2 • O • AlPO4 • NaCl • C6H5Cl • CuO

  4. Determine the number of steps for the following problems (1, 2, or 3): Given the following equation: 2 KClO3 –> 2 KCl + 3 O2 • How many moles of O2 can be produced by letting 12.00 moles of KClO3 react? • How many grams of O2 can be produced by letting 34.7g of KClO3 react? • How many moles of O2 can be produced by letting 14.6g of KClO3 react?

  5. Create the following mole ratios: • __Ag(s) + __H2S(g) + __O2(g) __Ag2S(s) + __H2O(l)(Equation must first be balanced.) • Ag : H2S • O2 : Ag2S • Ag2S : H2O • O2 : H2S • Ag : O2 • H2O : H2S How many ratios can this equation form?

  6. What is the molar ratio of all elements/compounds shown?

  7. Solve the following: Given the following equation: 2 KClO3 –> 2 KCl + 3 O2 • How many moles of O2 can be produced by letting 12.00 moles of KClO3 react?

  8. Solve the following: Given the following equation: 2 KClO3 –> 2 KCl + 3 O2 • How many grams of O2 can be produced by letting 34.7g of KClO3 react?

  9. Solve the following: Given the following equation: 2 KClO3 –> 2 KCl + 3 O2 • How many moles of O2 can be produced by letting 14.6g of KClO3 react?

  10. Solve the following: Given the following equation: Al2(SO3)3 +  6 NaOH  3 Na2SO3  +  2 Al(OH)3 • If 10.0 g of Al2(SO3)3 is reacted with 10.0 g of NaOH, determine the  limiting reactant

  11. Solve the following: Given the following equation:2 FePO4 + 3 Na2SO4 1 Fe2(SO4)3 + 2 Na3PO4 • What is the percent yield of this reaction if takes place with 25g of FePO4and an excess of Na2SO4, and produces 18.5g of Fe2(SO4)3

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