http://www.ck12.org Chapter 11. Chemical Reactions
Lesson Review Questions
- Categorize the following chemical reactions as single replacement, double replacement, combustion, combi-
nation, or decomposition.
a. Equimolar (having the same number of moles) solutions of silver nitrate and potassium chloride are
mixed to produce solid silver chloride and aqueous potassium nitrate.
b. Magnesium metal is added to hydrochloric acid to produce hydrogen gas and aqueous magnesium
chloride.
c. Ethanol is burned in air to produce water and carbon dioxide gas.
d. Water is electrolyzed to produce hydrogen and oxygen gas.
e. Hydrogen gas and oxygen gas are ignited to produce water. - Write the balanced chemical equation for the following combination and decomposition reactions.
a. Magnesium carbonate is heated strongly to produce magnesium oxide and carbon dioxide gas.
b. Hydrogen peroxide decomposes to produce water and oxygen gas.
c. Solid potassium chlorate is heated in the presence of manganese dioxide as a catalyst to produce potas-
sium chloride and oxygen gas. (Catalysts speed up reactions but are not expressed in the overall balanced
equation)
d. Molten aluminum oxide is electrolyzed using inert (non-reactive) electrodes to produce aluminum metal
and oxygen gas. - Write the balanced chemical equations for the following replacement reactions:
a. Zinc metal is added to a solution of iron(II) sulfate.
b. Equimolar solutions of lead(II) nitrate and sodium chloride are mixed to produce solid lead(II) chloride
and aqueous sodium nitrate.
c. Solutions of potassium phosphate and zinc nitrate are mixed. - Write the balanced chemical equations for the following combustion reactions.
a. Propane (C 3 H 8 ) is ignited in air to produce water and carbon dioxide gas.
b. Methanol(CH 4 O) is ignited in air to produce water and carbon dioxide gas.
c. Ethanol (C 2 H 5 OH) is burned in air. - Write the molecular equation, ionic equation, and net ionic equation for each of the following double replace-
ment reactions.
a. Silver nitrate reacts with potassium iodide to produce potassium nitrate and silver iodide.
b. Silver nitrate reacts with iron(III) chloride to produce iron(III) nitrate and silver chloride.
c. Lead(II) nitrate reacts with potassium iodide to produce potassium nitrate and lead(II) iodide.
d. Iron(III) chloride reacts with lead(II) nitrate to produce lead(II) chloride and iron(III) nitrate.
e. Calcium chloride reacts with sodium hydroxide to produce calcium hydroxide and sodium chloride. - Would it be possible to have a double precipitate formed for a double replacement process? Can you write an
equation where a double precipitate forms? - What is meant when we describe a compound as (aq) or (s)? Explain the similarities and differences between
these terms. - Write the balanced chemical equation for the combination reaction in which hydrogen and oxygen gases react
explosively to produce water. (Remember that hydrogen and oxygen exist as diatomic gases in their most
common elemental form.) - Write the balanced chemical equation for the reaction that occurs when a piece of aluminum metal is placed
in a solution of silver nitrate. - Using the solubility rules given above, predict whether or not the following compounds are soluble or insoluble
in water.