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|Chapter 4 and 5 Review |Leader: |Seth |

|Supplemental Instruction | | |

|Iowa State University | | |

| |Course: |Chem 177 |

| |Instructor: |Miller |

| |Date: |12/3/09 |

Announcements

1. Please fill out the SI evaluation survey online. Go to , scroll to the bottom of the page and select the link “Evaluation for Individuals Who Did/Did Not Attend SI Sessions”

2. The Chemistry Club will be selling the ACS Study Guides on Wednesday and Friday outside of the lecture halls before and after class. The cost of the Study Guide is $15. Cash only. Since Chem 177 is having an ACS standardized exam as part of your final exam, this Study Guide will help you earn a good grade on your exam.

3. Next session: Tuesday, 12/8/09

7:10-8 PM

1106 Pearson

4. Go around question- What is your favorite holiday?

Warmup Question: Reduction-oxidation

For the following equation:

[pic]

Which element is being oxidized and which is being reduced?

Which element is the oxidizing agent and which is the reducing agent?

Calculate the oxidation states.

What is the concentration of OH- when 25.0 mL of 3.5M NaOH are mixed with 30.0 mL of 1.7M Ca(OH)2?

| | |

|Element |Specific heat (J/goC) |

|Au |0.129 |

|Fe |0.444 |

10.0g of Au initially at 18.0oC is placed on 20.0g Fe at 55.6 oC. What is the final temperature of the two metals? Assume no heat is lost to the surroundings.

Define:

a) Molarity

b) Specific heat

c) The net ionic equation

d) Spectator ion

e) Enthalpy

f) Endothermic reaction

g) Exothermic reaction

If 20.0 g of solid NaOH are added to 1000 mL of a solution containing 0.500 moles of HCl, the temperature of the solution rises 6.9oC. Assuming that the total solution mass is 1000 g and the specific heat of the solution is 4.184 J/goC, calculate the heat released by this reaction. Then calculate ΔHrxn (i.e., the heat released per mole of NaOH).

What is the specific heat of a substance that absorbs 2.5 x 103 joules of heat when a sample of  1.0 x 104 g of the substance increases in temperature from 10.0C to 70.0C?

A solution is prepared by dissolving 14.7 g ammonium sulfate in enough water to make 106.0 mL of stock solution. A 12.40 mL sample of this stock solution is added to 52.10 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.

Aluminum reacts with an aqueous solution containing excess copper (II) sulfate.  If 1.85 g Al reacts and the percentage yield of Cu is 56.6%, what mass of Cu is produced?

Find ΔHrxn for 2SO2(g) +O2(g)[pic]2SO3(g)

[pic]

Wrap up

Write down what you learned today.

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