Review Sheet – Chemistry – Ch



Review Sheet – Chemistry, CCP – Ch. 12: Stoichiometry

Name: ______ANSWER______________ Date:___________ Period:___

This test covers materials in the textbook in Chapter 12 (p. 352-377). You are always responsible for the topics on the previous tests.

Test Expectations

The student should be able:

• Perform stoichiometry calculations starting with known quantities of moles, mass or volume and finding volume, mass, and moles using the information provided by a balanced chemical equation, including limiting reactant situations.

• Determine the limiting reactant of chemical reaction.

• Calculate percent yield of a chemical reaction given measured yields.

• Use stoichiometry calculations to show that chemical reactions obey the Law of Conservation of Matter (Mass).

1. Define each of the following terms clearly and completely.

a) stoichiometry –

b) limiting reagent/reactant –

c) nonstoichiometric proportions –

d) conservation of mass –

e) percent yield –

f) excess –

2. How many moles of water can be formed when 4.22 moles of ethane (C2H6) burn?

2 C2H6 + 7 O2 ( 4 CO2 + 6 H2O (moles-moles problem)

4.22 mol ? mol

[pic]

3. How many liters of carbon dioxide at STP can be produced by decomposing 47.4 grams of calcium carbonate?

CaCO3 ( CaO + CO2 (mass-volume problem)

47.4 g ? L

[pic]

4. How many liters of hydrogen are needed to react with 8.0 liters of nitrogen to produce ammonia (NH3)?

3 H2 + N2 ( 2 NH3 (volume-volume problem)

? L 8.0 L

[pic]

5. How many grams of copper(II) hydroxide are needed to form 100 grams of copper(II) oxide?

Cu(OH)2 ( CuO + H2O (mass-mass problem)

? g 100 g

[pic]

6. How many grams of NaCl can be formed if 24.8 grams of Na are allowed to react with 35.0 grams of Cl2?

2 Na + Cl2 ( 2 NaCl (limiting reactant problem)

24.8 g 35.0 g ? g

[pic]

[pic]

Pick the smallest, which is 57.8 grams.

7. The theoretical yield of a reaction was 3.74 grams of NaCl. One lab group obtained 3.57 grams NaCl. What was their percent yield?

[pic]

8. What is the theoretical yield if 15.0 grams of Zn are reacted with 31.9 grams of HCl and 10.6 grams of ZnCl2 are recovered?

Zn + 2 HCl ( ZnCl2 + H2 (limiting reactant/percent yield)

15.0 g 31.9 g ? g

[pic]

[pic]

[pic]

................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download