Name: ____________________________________________
Date: ____________________
Unit 7 Chemistry - Nail Lab
Purpose After you have completed the lab, think about what was the overall point for
performing the lab. What were we trying to accomplish?
Procedure
Day 1
1. Mass a clean & labeled _____________ mL beaker.
2.
Put between _________________ g of copper (II) chloride in the beaker. Record the mass of
the beaker and the copper (II) chloride.
3.
Add _______ mL of distilled water to the beaker. Stir to dissolve the solid.
4.
Obtain the mass of ________________ iron nails together to ± 0.01g.
5.
Place the nails in the copper (II) chloride solution. Observe the reaction; record your
observations. Place the labeled beaker in the place designated by your teacher.
Day 2
6. Remove the nails. Rinse or scrape the ________________________ (copper metal) from the
nails into your labeled beaker. Place the nails in a separate labeled small beaker. Note the
appearance of the nails in your observations. Place this beaker in the drying oven.
7.
___________________________ the solution from the 250 mL beaker. Rinse the precipitate
with about __________mL of distilled water. Try to lose as little of the solid copper as you can
when you decant. After a 2nd rinse with distilled water, rinse the copper with
_________________________________. Rinse one last time with distilled water. Then place
the labeled beaker in the drying oven.
8. Mass the dry nails, and then discard the nails.
Day 3
9. Mass the beaker + dry copper. Discard the copper in the place designated by your teacher. Wash
your beaker and let dry.
Data:
Mass 250 mL beaker
Mass 250 mL beaker + copper (II) chloride
Mass nails before reaction
Mass nails after reaction
Modeling Chemistry
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U6 nail lab v2.0
Mass 250 mL beaker + dry copper
Observations (For days 1, 2, & 3)
Calculations: Be sure to use correct units & significant figures in your work!
1.
Determine the mass of iron used during the reaction.
2.
Calculate the moles of iron used during the reaction.
3.
Determine the mass of copper produced by the reaction.
4.
Calculate the moles of copper produced by the reaction.
5.
Determine the ratio
6.
Express this ratio as an integer. For example, a ratio of 1.33 can be expressed as
expressed as
moles of copper.
moles of iron
2
, etc.
3
4
; 0.67 can be
3
Conclusion:
1.
In words, write down the reactions that occurred. (Hint: Look at the 2 reactants and the
product that is mentioned during the lab. A second product was made that was found in the
liquid you decanted – what must that product have been?)
2.
Even if you left the nails in the solution longer, no more copper would have formed. This
means that the reaction has stopped? Why did the reaction stop? Which reactant was used up?
How do you know?
3.
Describe what was happening to the atoms of iron and copper during the reaction. What is this
type of reaction called?
4.
What would happen to the ratio of copper produced to iron used if you had placed more nails in
the beaker? Explain your answer.
5.
What would happen to the ratio of copper produced to iron used if you let the reaction go for
less time? Explain your answer.
6.
If you were told that the accepted ratio of moles of copper produced to moles of iron used in this
reaction was supposed to be a 1:1 ratio, calculate your percent error. Account for differences
between your experimental value and the accepted value.
7.
Since iron can have a +2 or a +3 charge, there are two possible equations that could have
occurred depending on that charge (when you consider the 2nd product). Write the two possible
balanced equations for the reaction.
Modeling Chemistry
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U6 nail lab v2.0
Modeling Chemistry
3
U6 nail lab v2.0