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| Understanding the concepts
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Check your answers |
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| 1.
| Open the Information Conveyed by the Balanced Equation for the Production of Methanol Table on the Web site. If 20 molecules of H2 are reacted, how many molecules of CH3OH can be produced? If 2.5 mol of CO(g) are reacted, now many mol of H2 react?
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| 2.a.
| Typical chemical reaction problems involve calculating masses of reactants or products. What conversion factors are necessary to perform these calculations? |
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| 2.b.
| A balanced equation is critical for calculating the correct answer to these types of problems. Always make sure your equation is balanced. For practice balancing equations and then calculating masses of reactants or products, do Problems 9.26 and 9.32 in the text. |
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| 3.
| What are limiting reactant problems? Open the Limiting Reactant Understanding Concepts on the CD to examine limiting reactant problems on the microscopic level. After going through the introduction and example problem, do the Exercises. For each exercise, work through the problem before clicking the Hints. Click New Selection to get a new combination of reactant molecules for that reaction, or click Exercises to choose a different reaction. |
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| 4.
| In the macroscopic world, huge numbers of molecules are reacted. For these problems, moles of molecules should be used to determine limiting reactants. The most difficult part of limiting reactant problems is determining which reactant is limiting. What does it mean when we say a specific reactant is limiting?
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| 5.
| What is the theoretical yield? Give a reason why the actual yield is less than the theoretical yield. When a manufacturer is determining the best way to produce a certain chemical, will the most efficient reaction have a high or low percent yield? Explain. |
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| 6.
| Open Key Words on the CD and test your ability to define important terms presented in Chapter 9. |
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| 7.
| Test your understanding of Chapter 9 by taking the ACE quizzes on the Web site. |
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