Name: ______Date: ______

Unit 7 Chemistry - Nail Lab

PurposeAfter you have completed the lab, think about what was the overall point for performing the lab.

Procedure

Day 1

1.Mass a clean & labeled ______mL beaker.

2.Put between 6.0 - 8.5 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 2 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 precipitate (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.Decant the solution from the 250 mL beaker. Rinse the precipitate with about 25 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 25 mL of 1 M HCl. 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: make data table in lab NB

Mass 250 mL beaker
Mass 250 mL beaker + copper(II) chloride
Mass nails before reaction
Mass nails after reaction
Mass 250 mL beaker + dry copper

Observations (For days 1, 2, & 3) in lab NB

Calculations:Be sure to use correct units & significant figures in your work! Show all work in lab NB.

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 ofcopperproduced by the reaction.

5.Determine the ratio moles of copper.

moles of iron

6. Express this ratio as an integer. For example, a ratio of 1.33 can be expressed as ; 0.67 can be expressed as , etc.

Conclusion: in complete, legible sentences in lab NB.

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 Chemistry1U6 nail lab v2.0