Name
Class
Date
Single Replacement Lab
Background Information: Chemical reactions involve the rearrangement of elements to form new
compounds. According to the law of conservation of matter, (nothing can be created or destroyed), the products
we end up with must have the same number of atoms as the reactants we started with. Single replacement
reactions occur when one element replaces another element in a compound. This results in a new compound
and a different “free” element than the one we started with.
General formulas for single replacement reactions:
A + BC  AC + B
D + BC  BD + C
(the positive ion (B) is replaced with (A))
(the negative ion (C) is replaced with (D))
For example: Aluminum plus silver sulfide yields aluminum sulfide plus silver
2Al + 3AgS  Al2S3 + 3Ag
Objective: To determine if one metal can replace another in a compound.
Problem: How can one metal replace another metal in a compound?
Hypothesis:
Materials: (list materials used)
Procedure:
1. Collect 3 test tubes, rack, and samples of zinc (Zn), iron (Fe), and copper (Cu).
2. Half fill 2 test tubes with copper sulfate (CuSO4) solution. Label each as “A”CuSO4 ,“B” CuSO4.
3. Half fill 1 test tube with silver nitrate (AgNO3) solution. Label the test tube AgNO3.
4. Record observations of all materials before the reaction.
5. Place a zinc sample (Zn) in one of the copper sulfate solutions.
6. Put an iron sample (Fe) into the other copper sulfate solution.
7. Put a copper sample (Cu) into the silver nitrate solution.
8. Leave all test tubes for 5 minutes and record observations during the reaction.
9. Leave all test tubes overnight then record observations after the reaction.
Data: (Record detailed observations)
Appearance, color etc., of the copper sulfate solution (CuSO4):
Before reaction:
During reaction:
After reaction:
Appearance, color etc., of the silver nitrate solution (AgNO3):
Before reaction:
During reaction:
After reaction:
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Appearance, color etc., of the copper sulfate solution (CuSO4):
Before reaction:
During reaction:
After reaction:
Appearance, color etc., of the iron sample (Fe):
Before reaction:
During reaction:
After reaction:
Appearance, color etc., of the zinc sample (Zn):
Before reaction:
During reaction:
After reaction:
Appearance, color etc., of the copper sample (Cu):
Before reaction:
During reaction:
After reaction:
Conclusion:
Thought Questions:
1. What is the definition of a single replacement reaction?
2. What changes did you observe in the iron sample during the reaction?
What metal formed on the iron nail?
Where did this new metal come from?
3. What changes did you observe in the zinc sample during the reaction?
What metal formed on the zinc strip?
Where did this new metal come from?
4. What changes did you observe in the copper sample during the reaction?
What metal formed on the copper strip?
Where did this new metal come from?
5. Fill in the following formulas for the reactions that took place in each of the test tubes during this
experiment:
CuSO4 + Fe 
CuSO4 + Zn 
AgNO3 + Cu 
Summary: (Use three paragraph format to summarize your findings).
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