9.1 Review
Name__________________________
Stoichiometry: Mole-Mole Problems
Period______Date________________
Completion: Complete the following sentences by filling in the appropriate word or phrase from the list
below. Each word or phrase may be used once, more than once, or not at all.
reactants
particles
actual
subscripts
coefficients
quantitative
conservation of matter
mass
molar ratio
1. Stoichiometry is the study of the ______________________________ relationships that exist in
chemical reactions.
2. Stoichiometry can be used to determine how much product will form from a given amount of
__________________________.
3. The ____________________________ in a balanced equation indicate(s) the number of particles
of each substance taking place in the reaction.
4. It is possible to interpret the coefficients in a balanced chemical equation as either the number of
moles or the number of _________________________ involved in the reaction.
5. The coefficients in an equation do not show the _____________________ number of moles, only
the relative number involved.
6. You must determine the ___________________________ in a balanced equation before solving
any stoichiometry problem.
7. A balanced equation verifies the Law of ____________________________________________.
True & False: If the statement is true, write “true.” If it is false, change the underlined word or words to
make the statement true. Write your answer on the line provided.
__________________8. The term stoichiometry is derived from the Greek words stoicheion, meaning
element, and metron, meaning measure.
__________________9. You can determine the number of moles of any substance produced in a reaction
if you know the number of moles of at least two of the reactants.
__________________ 10. The molar ratio of hydrogen to oxygen in the equation
2H2 + O2 → 2H2O is 1:2.
__________________11. The total mass of the reactants is equal to the total mass of the products in a
chemical reaction.
__________________12. Mole-mole problems involve conversions from moles of one substance to
mass of another.
Problems: Solve each of the following problems as directed. Show all your work.
13. How many moles of magnesium are required to react 2.0 mol of hydrochloric acid in a single
replacement reaction? Write the balanced equation and solve the problem.
14. Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. Write the
balanced equation for this reaction and calculate the number of moles of hydrochloric acid required to
react with 0.87 mol of Al.
15. Glucose (C6H12O6) combines with oxygen gas in the body in a combustion reaction to produce
carbon dioxide gas and water. Write the balanced equation for this reaction. How many moles of
oxygen gas are required to combine with 0.25 mol of glucose? How many moles of carbon dioxide
gas and water would be produced by this reaction?
16. Calcium carbonate combines with hydrochloric acid to produce calcium chloride, water and carbon
dioxide gas. Write the balanced equation for this reaction. How many moles of hydrochloric acid are
required to react with 2.5 mol of calcium carbonate? . How many moles of carbon dioxide would
be produced?
17. Zinc reacts with sulfuric acid in a single replacement reaction. How many moles of hydrogen gas will
be produced if 0.36 mol of zinc reacts completely?