Chemistry I
Chapter 6- Balancing Chemical Equations
Name:____________________________________
1. Choose the response that best answers the question “Why do we not change subscripts
when balancing a chemical equation?”
[A] It is fine to do once in awhile, but don’t make a habit of it.
[B] Compounds composed of the same elements and having different subscripts are
different substances.
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[C] There’s no real reason not to, it’s just something that is not done.
[A] Mendeleev
[B] Dalton
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[C] Chadwick
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2. Who is responsible for the atomic theory that makes it necessary to balance chemical
equations?
Balance the following equations. (1 points per blank, plus 2 points each if you get it correct)
(example #3- 3+2 = 5 total points)
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3. ____ N2 + ____ H2 Æ ____ NH3
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4. ____ KClO3 Æ ____ KCl + ____ O2
5. ____ NaCl + ____ F2 Æ ____ NaF + ____ Cl2
Chemistry I
Chapter 6- Balancing Chemical Equations
Name:____________________________________
6. ____ Pb(OH)2 + ____ HCl Æ ____ H2O + ____ PbCl2
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8. ____ CH4 + ____ O2 Æ ____ CO2 + ____ H2O
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7. ____ AlBr3 + ____ K2SO4 Æ ____ KBr + ____ Al2(SO4)3
9. ____ C3H8 + ____ O2 Æ ____ CO2 + ____ H2O
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10. ____ C8H18 + ____ O2 Æ ____ CO2 + ____ H2O
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11. ____ FeCl3 + ____ NaOH Æ ____ Fe(OH)3 + ____NaCl
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12. ____ P + ____O2 Æ ____P2O5
13. ____ Na + ____ H2O Æ ____ NaOH + ____H2
14. ____ Ag2O Æ ____ Ag + ____O2
Chemistry I
Chapter 6- Balancing Chemical Equations
Name:____________________________________
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16. ____ K + ____ MgBr Æ ____ KBr + ____ Mg
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15. ____ CO2 + ____ H2O Æ ____ C6H12O6 + ____O2
17. ____ HCl + ____ CaCO3 Æ ____ CaCl2 + ____H2O + ____ CO2
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18. ____ HNO3 + ____ NaHCO3 Æ ____ NaNO3 + ____ H2O + ____ CO2
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19. ____ H2O + ____ O2 Æ ____ H2O2
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20. ____ NaBr + ____ CaF2 Æ ____ NaF + ____ CaBr2
21. ____ H2SO4 + ____ NaNO2 Æ ____ HNO2 + ____ Na2SO4
Answer the following questions with a word, phrase or sentence. ( 1 point each)
Chemistry I
Chapter 6- Balancing Chemical Equations
Name:____________________________________
22. Where are products located in a reaction (left or right of arrow)?
23. Where are reactants located in a reaction (left or right of arrow)?
24. In a chemical equation, what does this Æ mean?
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What are the 4 states of matter descriptions used in chemical equations and what symbol is used
to represent each?
25.
26.
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27.
28.
Name 5 possible indications that a chemical reaction may have taken place.
29.
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30.
32.
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33.
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31.
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34. What is the determining factor as to whether or not a chemical reaction has taken place?
35. Why is it necessary to balance a chemical equation? (2 points)
Write and balance the following equations. Be sure to include states of matter!!
Chemistry I
Chapter 6- Balancing Chemical Equations
Name:____________________________________
36. The reaction of ammonia (NH3) with chlorine to form nitrogen trichloride and hydrogen
gas.
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37. The combustion (means reacts with oxygen to form carbon dioxide and water) of propane
(C3H8).
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38. The incomplete combustion (means reacts with oxygen) of propane (C3H8) to form
carbon monoxide and water.
39. The reaction of nitric acid with sodium hydroxide to form sodium nitrate and water.
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40. The reaction of copper (II) oxide with hydrogen to form copper metal and water.
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41. The reaction of aluminum metal with oxygen to form aluminum oxide.
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42. The complete combustion (means reacts with oxygen to form carbon dioxide and water)
of 2,2-dimethylpropane (C4H10) in oxygen.
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43. The reaction of iron (III) bromide with magnesium hydroxide to produce magnesium
bromide and iron (III) hydroxide.
44. The decomposition of hydrogen peroxide to form water and oxygen.
45. The reaction of ammonia (NH3) with sulfuric acid to produce ammonium sulfate.
Chemistry CP
Chapter 7 Test
Name:______________________________
Please answer the following questions with a word or phrase. (2 points each)
1. What do acid-base reactions always form?
2. What do precipitation reactions always form?
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3. What type of reaction transfers electrons?
4. What is a spectator ion?
Explain the five reaction types: COMBUSTION, DECOMPOSITION, DOUBLE
5. Combustion:
6. Decomposition:
7. Double Displacement:
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8. Single Displacement:
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the reaction
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DISPLACEMENT, SINGLE DISPLACEMENT, SYNTHESIS, with regard to what happens in
9. Synthesis:
10. What is transferred in an oxidation reduction reaction?
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11. The formation of a gas is accompanied at least one of which two other driving forces?
12. What two processes occur simultaneously to transfer electrons?
For the following equation, write the COMPLETE IONIC equation from the given molecular
equation. (4 points)
13. Na2SO4 (aq) + Ba(NO3)2 (aq)  NaNO3 (aq) + BaSO4 (s)
Chemistry CP I
Chapter 7 TEST
Name: _______________________________
14. When a precipitation reaction occurs, What happens to the ions that do NOT form the
precipitate?
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15. An aqueous solution of barium nitrate is reacted with an aqueous solution of sodium
sulfate, which of the following substances would be the solid formed by the reaction.
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16. Which man developed the basic definitions of an acid and of a base?
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17. A substance that, when dissolved in water, completely dissociates (comes apart) into its
component ions is known as a _____________________.
Please indicate the DRIVING FORCE for each of the following unbalanced reactions. (3
points each) Use each driving force only ONCE!!!!
Driving Force
18. HCl (aq) + Mg (s)  MgCl2 (aq) + H2 (g)
________________________
19. H2SO4 (aq) + NaOH (aq)  Na2SO4 (aq) + H2O (l)
________________________
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Reaction
20. Ag(NO3)2 (aq) + KCl (aq)  KNO3 (aq) + AgCl (s)
________________________
21. Zn (s) + CuSO4 (s)  ZnSO4 (s) + Cu (s)
________________________
Chemistry CP I
Chapter 7 TEST
Name: _______________________________
Please indicate the type of reaction exemplified by the following equations by choosing a type
from the following: COMBUSTION, DECOMPOSITION, DOUBLE DISPLACEMENT,
SINGLE DISPLACEMENT, SYNTHESIS. Each choice is used only once! (3 points each)
_____________________________
23. H2O2 (l)  H2O (g) + O2 (g)
_____________________________
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22. C2H10 (g) + O2 (g)  CO2 (g) + H2O (l)
25. Mg (s) + O2 (g)  MgO (s)
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24. Na3PO4 (aq) + Ca(NO3)2 (aq)  NaNO3 (aq) + Ca3PO4 (s) ________________________
______________________________
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26. Al (s) + Fe2O3 (aq)  Al2O3 (aq) + Fe (s)
______________________________
Predict the products of the following reactions. (3 points each)
27. HCl (aq) + KOH (aq)  _______________________ + _________________________
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28. HCl (aq) + Zn (s) _______________________ + _________________________
29. H2 (s) + O2 (g)  _______________________
30. CH4
(g)
+ O2 (g)  _______________________ + _________________________
Chemistry CP I
Chapter 7 TEST
Name: _______________________________
Complete following equations by predicting the products, include the states of matter. Circle
Reaction or No Reaction to indicate if the reaction actually occurs. 4 points each
31. Na2S (aq) + KCl (aq)  ________________________ + __________________________
NO REACTION
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REACTION
32. Ag(NO3)2 (aq) + NaCl (aq)  _______________________ + ___________________________
REACTION
NO REACTION
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33. Na3PO4 + K2SO4 (aq)  ________________________ + ___________________________
REACTION
NO REACTION
34. Na2S (aq) + ZnCl2 (aq)  __________________________ + _____________________________
NO REACTION
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REACTION
35. Pb(NO3)2 (aq) + Na2CO3 (aq)  _______________________ + ___________________________
REACTION
NO REACTION
For the following equations, write the NET IONIC equation from the given molecular equation.
(3 points each)
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36. Pb(NO3)2 (aq) + K2S (aq)  KNO3(aq) + PbS (s)
37. KOH (aq) + H2SO4(aq)  H2O (l) + K2SO4 (aq)
Chemistry CP I
Chapter 7 TEST
Name: _______________________________
Please answer the following thought provoking question. Please ask if you do not understand
the question. (6 points)
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38. You need to create a working “volcano” for science class. The chemicals you have
available are: Na2CO3 (s) , NaOH(s) and HCl (aq). In order to produce the desired
volcano effect you will need to produce a gas. Which two chemicals will produce a gas
when mixed? Using you knowledge of chemical reactions, explain, USING CHEMISTRY
TERMS AND EQUATIONS, which chemicals to mix AND WHY. Hints: React each of
the solids with the HCl. Remember H2CO3 splits into H2O and CO2.
NaOH Reaction:
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Na2CO3 Reaction:
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Which chemicals should you use and Why: