Lab: Mole Ratio
Name:
Period: _______
Iron reacts with copper sulfate in a single displacement reaction. By measuring the mass
of iron that reacts with the mass of copper metal produced, you can calculate the ratio of
moles of product. This mole ratio can be compared to the ratio found in the balanced
equation.
Mass of empty 150 mL beaker
_________________
Mass of 150 mL beaker + CuSO4
_________________
Mass of CuSO4
_________________
Mass of iron filings
_________________
Mass of beaker with dried copper
_________________
Mass of dried copper
_________________
Procedures
1. Put your safety glasses and aprons on.
2. Measure and record the mass of a clean dry beaker.
3. Place about 12 g of copper sulfate in to the beaker and weigh and record the
combined mass.
4. Add 50 mL of water to the copper sulfate and heat the mixture on the hot plate at
a setting of “5”. Stir until the entire solid is dissolved, but do not boil. Using
tongs, remove the beaker from the hot plate.
5. Measure about 2 grams of iron filings onto a piece of weighing paper. Measure
and record the exact mass of the filings.
6. While stirring, slowly add the iron filings to the hot copper sulfate solution.
7. Allow the reaction to stand, without stirring for 5 minutes to insure complete
reaction. The solid copper metal will settle to the bottom of the beaker.
8. Pour off the liquid into a 400mL beaker, being careful to leave the copper solid on
the bottom of the 150 mL beaker.
9. Add 15 mL of water to the beaker with the copper solid and carefully swirl the
beaker to wash the copper. Pour the water into the 400 mL beaker, being careful
to leave the copper solid in the bottom of the 150 mL beaker.
10. Repeat step 8 two more times.
11. Place the 150 mL beaker containing the wet copper on the hot plate and dry the
copper at a setting of “5”.
12. After all the water has evaporated, remove the beaker form the hot plate and allow
it to cool for 5 minutes.
13. Measure and record the mass of the 150 mL beaker and the copper.
14. Turn the hot plate off, place the dry copper in a kill jar, clean the beakers, clean
your lab station, and wash your hands.
Over
Questions
1. What evidence do you have that a chemical reaction took place?
2. Write a balanced equation for the chemical reaction that occurred.
3. From your data determine the mass of copper produced.
4. Use the mass of the copper to calculate the moles of copper produced.
5. Calculate the moles of iron used in the reaction.
6. Divide the moles of iron by the moles of copper to determine the whole number
ratio of iron to copper.
7. Compare the ratio of moles of iron to moles of copper from the balanced chemical
equation to the mole ratio calculated using your data.
8. Which substance was the limiting reactant in this equation?