Ch 100: Final Exam Review Information



Ch 100: Exam #3 Review Information

Exam will be given at 10:00 a.m., Mar. 19, 2007 (Tuesday) in JH Room 107

Exam will be roughly 1 hour in length

bring a scientific calculator & a single-sided (3” x 5”) sheet of notes

Information Provided:

Periodic Table

Table of atomic masses

Solubility Chart

Notes:

Exam will cover chapters 7 (all), 8 (8.1-8.5), 9 (9.1-9.3)

Go over assigned reading and homework as well as lecture notes

Go over class worksheets (the answer keys are at MyPCC)

Specific Study Points:

Ch 7: precipitation reactions & prediction of solid(s) formed, types of chemical equations (molecular, complete ionic & net ionic), spectator ions, describe oxidation-reduction reaction, classifying chemical reactions, strong vs. weak electrolytes

Ch 8: the mole & Avogadro’s number, calculate grams from moles, calculate moles from # of atoms/molecules, calculate grams from # of atoms/molecules, calculate mass percent of element in a compound

Ch 9: mole-mole relationships in chemical reactions

Ch 14: mass concentration and molar concentration

Notes:

1. Aqueous Chemical Reactions & Predicting Solubility

2. Types of chemical equations: molecular, complete and net ionic equations

3. Types of Chemical Reactions

4. The Mole & Avogadro’s Number ( calculate grams from moles, moles from grams

5. Percent composition (mass or volume)

6. Mole-Mole relations in chemical reactions

Practice Problems:

1. From the following reaction, 200.0 grams of magnesium chloride were produced from elemental magnesium and gaseous chlorine:

Mg (s) + Cl2 (g) ( MgCl2 (s)

(i) How many moles of magnesium chloride are produced by this reaction?

(ii) How many moles of Mg2+ are in the 200.0 g of MgCl2?

(iii) How many moles of Cl- are in the 200.0 g of MgCl2?

(iv) What is the percent composition of Cl in MgCl2?

2. In a “Zippo” cigarette lighter, the following unbalanced chemical reaction occurs:

C3H8 (g) + O2 (g) ( CO2 (g) + H2O (g)

i) Balance this reaction.

ii) During this reaction 5.0 moles of oxygen gas are consumed. How many moles of butane (C3H8) were burned in this reaction?

ii) How many moles of carbon dioxide were produced?

iii) How many moles of water were produced?

iv) How many different ways can you classify this reaction?

3. You dissolve 15.00 g of MgCl2 in de-ionized H2O to make 0.50 L of solution. How many moles of MgCl2, Mg2+ and Cl-, respectively, are in this solution?

4. A flask contains 0.2500 moles of aqueous KOH in solution.

i) What is the molar mass of KOH?

ii) How many grams of KOH, K, O and H, respectively, are in this solution?

iii) What is the percent composition of each ion (i.e. K+ and OH-), respectively, in KOH?

5. The “active” ingredient in common household bleach is sodium hypochlorite. Answer the following questions for a pure sample of sodium hypochlorite.

i) What is the chemical formula for sodium hypochlorite?

ii) What is the molar mass?

ii) What is the percent composition (by mass) of each element?

iii) What is the percent composition (by mass) of each ion, respectively, in sodium hypochlorite?

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