Download Lesson Review Questions

Lesson Review Questions
1. Categorize the following chemical reactions as single replacement, double replacement,
combustion, combination, 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.
2. 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 potassium 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.
3. 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.
4. Write the balanced chemical equations for the following combustion reactions.
a. Propane (C3H8) is ignited in air to produce water and carbon dioxide gas.
b. Methanol(CH4O) is ignited in air to produce water and carbon dioxide gas.
c. Ethanol (C2H5OH) is burned in air.
5. Write the molecular equation, ionic equation, and net ionic equation for each of the following
double replacement reactions.
a.
b.
c.
d.
e.
Silver nitrate reacts with potassium iodide to produce potassium nitrate and silver iodide.
Silver nitrate reacts with iron(III) chloride to produce iron(III) nitrate and silver chloride.
Lead(II) nitrate reacts with potassium iodide to produce potassium nitrate and lead(II) iodide.
Iron(III) chloride reacts with lead(II) nitrate to produce lead(II) chloride and iron(III) nitrate.
Calcium chloride reacts with sodium hydroxide to produce calcium hydroxide and sodium
chloride.
6. 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?
7. What is meant when we describe a compound as (aq) or (s)? Explain the similarities and
differences between these terms.
8. 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.)
9. Write the balanced chemical equation for the reaction that occurs when a piece of aluminum
metal is placed in a solution of silver nitrate.
10. Using the solubility rules given above, predict whether or not the following compounds are soluble
or insoluble in water.
a. Potassium nitrate
b. Lead(II) chloride
c. Barium sulfate
d. Aluminum sulfide
e. Calcium carbonate