NAME _____________________________________________
PERIOD ________
DATE __________________________
Chapters 9-10 Test Review
Reminders: Show all work and units. Round all decimal answers to TWO decimal places. You are
welcome to use one 3x5 card (front and back) on the test.
Questions #1-10 are True or False. Write TRUE or FALSE on the blank next to each question.
1. _________ Chemical equations must be balanced to satisfy the law of conservation of mass.
2. _________ The reaction type in which oxygen reacts with another substance, often producing
heat, light, water, and carbon dioxide is a decomposition reaction.
3. _________ The reaction type in which a single compound is broken down into simpler
substances is called a decomposition reaction.
4. _________ Fluorine, iodine, oxygen, hydrogen, and nitrogen will be found as diatomics in
nature.
5. _________ The reaction type in which two or more substances combine to form a single
compound is a synthesis reaction.
6. _________ A catalyst speeds up a reaction but is not actually used in the reaction itself.
7. _________ The symbol (s) means that a salt was formed.
8. _________ The units for molar mass are g/L.
9. _________ The products in a chemical reaction are the starting substances.
10. _________ In order to convert grams to mol use Avogadro’s number.
11. Balance the following equations and then identify the type of reaction below:
a. ______ Al2(SO4)3 + ______ KOH
______ Al(OH)3 + ______ K2SO4
i. _______________________________________________
b. ______ Fe + ______ Cl2
______FeCl3
i. _______________________________________________
c. ______ Mg + ______H3PO4
______Mg3(PO4)2 + ______H2
i. _______________________________________________
d. ______ Fe2S3 + ______HCl
______ FeCl3 + ______ H2S
i. _______________________________________________
e. ______ C3H6 + ______ O2
______ CO2 + ______H2O
i. _______________________________________________
f. ______ Al(OH)3
______ Al2O3 + ______ H2O
i. _______________________________________________
g. ______ Ba(CN)2 + ______ H2SO4
______ BaSO4 + ______HCN
i. _______________________________________________
h. ______ C3H8 + ______ O2
______ CO2 + ______ H2O
i. _______________________________________________
i.
______ Ba(NO3)2 + ______ Na2SO4
i.
j.
______ BaSO4 + ______ NaNO3
_______________________________________________________________________
______ HgO
______ Hg + ______O2
i. ________________________________________________
12. Predict the products and balance the following chemical equations:
a. ______ Al + ______Cl2
___________________________________________
b. ______ Ag + ______ KNO3
c. ______ Fe(SO4)3 + _______ Ba(OH)2
d. ______ C6H12 + ______ O2
e. ______ Al + ______FeO
f. ______ C2H5OH + ______ O2
g. ______ H2 + ______ O2
h. ______ AlBr3 + ______ K2SO4
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i.
______ H2SO4 + ______ NaNO2
j.
______ NaCl + ______ F2
k. ______ K + ______ MgBr2
l.
______ MnO2 + ______ Sn(OH)4
m. ______ O2 + ______ C2H4O2
n. ______ NaOH + ______ H2SO4
o. ______ MgCl2 + ______Li2CO3
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13. Write and balance a chemical equation for the following word equations in the spaces below.
Note that for some of the equations you may need to also predict the products by writing both
the name of the compound(s) in the blank and by writing their formula(s) in the chemical
equations.
a. Butane (C4H10) reacts with oxygen gas to yield __________________________________
b. Barium chloride reacts with potassium chromate to form barium chromate and
potassium chloride.
c. Magnesium sulfide reacts with calcium to form _________________________________
d. Copper (II) oxide reacts with hydrogen gas to produce copper metal and water.
e. Iron metal reacts with oxygen gas to form iron (III) oxide.
f. Aluminum nitrate and sodium sulfide react to form ______________________________
g. Aluminum sulfate reacts with calcium hydroxide to yield aluminum hydroxide and
calcium sulfate.
h. Potassium metal reacts with water to produce potassium hydroxide and hydrogen gas.
i.
Dinitrogen pentoxide plus water gives nitric acid.
j.
Iron (II) sulfide reacts with oxygen to give iron (III) oxide and sulfur dioxide.
14. Write the (1) balanced chemical equation, (2) the balanced complete ionic equation, and (3) the
balanced net ionic equation for the following reactions:
a. H3PO4(aq) + Ca(OH)2(aq)
Ca3(PO4)2(aq) + H2O(l)
b. Aqueous potassium iodide reacts with aqueous silver nitrate to produce a silver iodide
precipitate and aqueous potassium nitrate.
c. Aqueous hydrochloric acid reacts with aqueous calcium hydroxide to produce liquid
water and aqueous calcium chloride.
15. How many molecules of NaCl are there in 0.150 mol NaCl (sodium chloride)?
16. How many Cu atoms are in 2.50 mol Cu?
17. How many moles are in 300.0 g S?
18. How many grams are in 3.57 mol Al?
19. How many atoms are in 0.230 g Pb?
20. How many grams are in 1.50 x 1015 N atoms?
21. What is the molar mass of CCl4?
22. How many moles are in 6.50 g of ZnSO4?
23. How many sulfite ions (SO32-) are present in a 2.25 g sample of sodium sulfite (Na2SO3)?
24. What is the percent composition of NaHCO3 (sodium hydrogen carbonate)?
25. What is the molecular formula for a compound that contains 46.68% N and 53.32% O and has a
molar mass of 60.01 g/mol?