2011-2012 Lv One Chemistry
Chapter 9:
Name __________________________________
Sulfate Lab
Stoichiometry
Iron and Copper(II)
In this lab you will react iron with copper(II) sulfate and measure
the amount of copper produced. You will then calculate the
theoretical yield of copper, and use these two values to determine
your percent yield.
Purpose: Record the overall purpose of this lab activity (what are we
trying to do and in general, how).
Chemical Reaction: Write a balanced chemical equation for the reaction
in this lab. Assume the iron in the product has a +2 charge.
Required Materials:
experiment
List all chemicals and supplies needed for the
Safety and Disposal: Use MSDS to identify the hazards of iron and
copper (II) sulfate. In addition, record any disposal instructions
indicated on the lab handout.
Procedure: Include a drawing of the set-up/apparatus.
Pre-lab Questions
1. Define the following terms in your own words: limiting reactant,
excess reactant and percent yield.
2. The following observations were recorded from the reaction of
aluminum metal and copper(II) chloride.
Before Reaction
During Reaction
After Reaction
Al – Is a silverReaction feels warm Some of the aluminum
colored shiny,
A red/brown solid
remains
opaque solid
is produced
there is a clear
colorless liquid in
CuCl2- is a clear
the beaker
blue liquid
Based on the observations above what is the limiting reactant in
this reaction? What is the excess reactant? Use data to support
your answer.
3. If 4.35 g of copper (II) sulfate (249.7 g/mol) is used in a
reaction with iron, what mass of copper should be produced?
4. You actually produced 0.96 g of copper in the situation
described in question 3. What is the percent yield of your
reaction?
Data Table: Construct a data table to record all required measurements
in the lab.
Observations: Construct an observations table to record all required
qualitative observations.
Procedure:
1. Measure out approximately 6 grams of copper (II) sulfate
2011-2012 Lv One Chemistry
Chapter 9:
Stoichiometry
pentahydrate (CuSO4  5H2O) in a plastic weighing tray. Record the
exact mass in your data table.
2. Add the copper (II) sulfate and approximately 50.0 mL of distilled
water in a 100-mL beaker. Record your observations of what happens
when the copper (II) sulfate is added to water.
3. Set up your heating apparatus, using your Bunsen burner, ring
stand, iron ring, and wire gauze. Gently heat the copper (II) sulfate
solution in the beaker without allowing it to boil. Continue heating
it, stirring occasionally with a glass stirring rod until all the
crystals are dissolved. Turn off the burner and place the beaker on
the lab bench and allow it to cool.
4. Measure approximately 1.00 g of iron filings in a plastic tray.
Record the exact mass of iron used in your data table.
5. While stirring, slowly add the iron to the heated copper (II)
sulfate solution.
6. Allow the beaker to sit for about 10 minutes while the reaction
progresses. Record your observations.
7. While you are waiting, write your names on a piece of filter paper,
then find and record the exact mass of the filter paper.
8. Fold the piece of filter paper in quarters and fit it snugly in the
funnel. Add a small amount of water from your wash bottle to help the
paper stick to the sides of the funnel.
9. Filter the mixture into an erlenmeyer flask.
Using the rubber policeman, stir the mixture vigorously. Then, pour
the mixture into the funnel. Scrape all of the solid into the funnel
using the rubber policeman. When all of the mixture has been poured
into the funnel, use a small amount of water to rinse the beaker into
the funnel. Using a small amount of water, rinse the solid in the
funnel to be sure all of the solution has drained through. Record your
observations of the solid on the filter paper and the liquid in the
flask after filtering.
11. Carefully, remove the damp filter paper from the funnel and lay it
flat on the lab bench. Allow the paper to dry overnight.
12. Clean all of the lab materials, your desk, and your hands. Dump
all of the remaining liquid into the waste container in the hood, Do
not pour it down the sink.
13. Day Two: Find and record the mass of the dried solid and the
filter paper. Your dried product can be disposed of in the trash.
Calculations:
1. Calculate the number of moles of copper (II) sulfate pentahydrate
used. The molar mass of copper (II) sulfate pentahydrate is 249.7
g/mol.
2. Calculate the number of moles of iron used.
3. Using stoichiometry, calculate the maximum number of grams of
copper that could theoretically be produced. Remember to start with
your limiting reactant!
4. Calculate the mass of copper actually produced.
5. Calculate the percent yield using the actual and theoretical masses
calculated above.
Error Analysis: Do not do a % error calculation. Provide at least
three possible sources of error AND explain how each one impacts your
results (what affect does the error have on your measured value(s),
2011-2012 Lv One Chemistry
Chapter 9:
Stoichiometry
and what is the effect on your percent yield?). Be sure this is well
written with full sentences.
Conclusion: Provide a brief (3-4 sentences) summary of your results
and how they relate to the scientific content being discussed in
class.
Title/Date
Purpose
Chemical Reaction
Required Materials
Safety & Disposal
Procedure
Pre-lab Questions
Data Table
Observations
Conclusion
Calculations
Error Analysis
Complete
without
errors
1
1
2
1
1
1
2
3
3
1
Proficient
7-6
7-6
Incomplete
or complete
with errors
0.5
0.5
1
0.5
0.5
0.5
1
2-1
2-1
.5
Developing
5-4
5-4
Missing
0
0
0
0
0
0
0
0
0
0
Beginning
3-1
3-1
Missing
0
0
Score: _________ /30