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AP Reactions Review
Name ______________________________________________ Period_____
For the following reactions write a net ionic equation. Box your final answer.
1. Carbon disulfide vapor is burned in excess oxygen.
a. What would be the products if the oxygen gas was not in excess?
2. Potassium permanganate solution is added to an acidic solution of hydrogen peroxide.
a. This reaction produces a gas. Describe an experimental test that you would use to test for and identify this gas, explaining the
expected results.
3. Propanol is burned completely in air.
a. This reaction produces a gas. Describe an experimental test that you would use to test for and identify this gas, explaining the
expected results.
4. Excess potassium hydroxide solution is added to a solution of potassium dihydrogen phosphate.
a. How does the oxidation number of phosphorus change in this reaction?
5. A solution of sodium hydroxide is added to a solution of ammonium chloride.
a. State the two acid-base pairs of this Bronsted-Lowry acid-base reaction.
6. Powdered magnesium carbonate is heated strongly.
a. Why does this reaction state “strongly”?
7. An excess of nitric acid solution is added to a solution of tetraamminecopper(II) sulfate, Cu(NH3)42+.
a. State the change in pH you would expect before and after this reaction. Explain.
8. Solid sodium oxide is added to water.
a. If phenolphthalein were added to the water before the reaction, what color change, if any would occur?
9. A concentrated solution of ammonium thiocyanate is added to a solution of iron(III) chloride.
a. Identify the Lewis acid and Lewis base.
10. A concentrated solution of ammonia is added to a solution of copper(II) chloride.
a. Is ammonia a Lewis acid or base? Explain.
11. A piece of lithium metal is dropped into a container of nitrogen gas.
a. If the container was sealed quickly, what would you expect to happen to the pressure inside the container as the reaction proceeds?
12. Powdered magnesium oxide is added to a container of carbon dioxide gas.
a. State the oxidation number of each element before and after the reaction.
AP Reactions Review
Name ______________________________________________ Period_____
For the following reactions write a net ionic equation. Box your final answer.
1. Carbon disulfide vapor is burned in excess oxygen.
a. What would be the products if the oxygen gas was not in excess?
2. Potassium permanganate solution is added to an acidic solution of hydrogen peroxide.
a. This reaction produces a gas. Describe an experimental test that you would use to test for and identify this gas, explaining the
expected results.
3. Propanol is burned completely in air.
a. This reaction produces a gas. Describe an experimental test that you would use to test for and identify this gas, explaining the
expected results.
4. Excess potassium hydroxide solution is added to a solution of potassium dihydrogen phosphate.
a. How does the oxidation number of phosphorus change in this reaction?
5. A solution of sodium hydroxide is added to a solution of ammonium chloride.
a. State the two acid-base pairs of this Bronsted-Lowry acid-base reaction.
6. Powdered magnesium carbonate is heated strongly.
a. Why does this reaction state “strongly”?
7. An excess of nitric acid solution is added to a solution of tetraamminecopper(II) sulfate, Cu(NH3)42+.
a. State the change in pH you would expect before and after this reaction. Explain.
8. Solid sodium oxide is added to water.
a. If phenolphthalein were added to the water before the reaction, what color change, if any would occur?
9. A concentrated solution of ammonium thiocyanate is added to a solution of iron(III) chloride.
a. Identify the Lewis acid and Lewis base.
10. A concentrated solution of ammonia is added to a solution of copper(II) chloride.
a. Is ammonia a Lewis acid or base? Explain.
11. A piece of lithium metal is dropped into a container of nitrogen gas.
a. If the container was sealed quickly, what would you expect to happen to the pressure inside the container as the reaction proceeds?
12. Powdered magnesium oxide is added to a container of carbon dioxide gas.
a. State the oxidation number of each element before and after the reaction.
Answers
Carbon disulfide vapor is burned in excess oxygen.
CS2(g) + O2(g) → CO2(g) + SO2(g) [or SO3(g)]
Potassium permanganate solution is added to an acidic solution of hydrogen peroxide.
MnO4- + H2O2 → Mn2+ + O2 + H2O
Propanol is burned completely in air.
C3H7OH(l) + O2(g) → CO2(g) + H2O(g)
Excess potassium hydroxide solution is added to a solution of potassium dihydrogen phosphate.
OH-(aq) + H2PO4-(aq) → PO43-(aq) + H2O
A solution of sodium hydroxide is added to a solution of ammonium chloride.
OH-(aq) + NH4+(aq) → H2O + NH3(aq)
Powdered magnesium carbonate is heated strongly.
MgCO3  MgO + CO2
An excess of nitric acid solution is added to a solution of tetraamminecopper(II) sulfate.
H+ + Cu(NH3)42+ → Cu2+ + NH4+
Solid sodium oxide is added to water.
Na2O(s) + H2O → Na+(aq) + OH-(aq)
A solution of ammonium thiocyanate is added to a solution of iron(III) chloride.
Fe3+(aq) + SCN-(aq) → Fe(SCN)2+(aq) [or Fe(SCN)63-(aq)]
A concentrated solution of ammonia is added to a solution of copper(II) chloride.
Cu2+ + NH3 → Cu(NH3)42+
A piece of lithium metal is dropped into a container of nitrogen gas.
Li(s) + N2(g) → Li3N
Powdered magnesium oxide is added to a container of carbon dioxide gas.
MgO(s) + CO2(g) → MgCO3(s)