1. Which metal is the strongest oxidizing agent in your activity table? Which me
ID: 972979 • Letter: 1
Question
1. Which metal is the strongest oxidizing agent in your activity table? Which metal in your table is the strongest reducing agent? Explain.
2. If you wanted to design a battery from relatively common, inexpensive, and not too toxic materials, that produced a voltage of about 1V, which cell reaction would you use?
3. A. Will metallic magnesium precipitate if a piece of tin is added to a 1.0 M solution of magnesium sulfate? Explain.
B. Will a piece of copper dissolve in a 1.0 M solution of Pb(NO3)2? Explain
HERE IS THE PROCEDURE WE FOLLOWED:
Procedure Part I
1. Obtain a 9 cm filter paper and make a cell template according to Figure 1. Do not fold the paper and use only pencil to draw on it. Do not erase.
2. Write on each sector (using pencil only) the chemical symbol of each metal used in the experiment, as shown in figure 1.
3. Place the cutout filter paper onto the lid of a clean, dry plastic Petri dish.
4. Use tweezers to transfer the appropriate metal pieces onto their dedicated sections of the paper, Note: you are using steel nails instead of pure iron wire in this experiment.
5. Place 1-2 drops of the appropriate metal ion solution onto the paper at the edge of each metal piece. Make sure that the metal is contacting the solution. Make sure that the ion solutions don’t bleed enough to contact each other.
6. Drop 1.0 M KNO3 in the center of the paper to act as a salt bridge. Allow the KNO3 solution to soak outward until it contacts all other wet areas.
7. Turn the voltmeter on and switch the dial to measure DC voltage. Set the range to 2V. Ag Cu Pb Fe g M l A Sn Ni KNO3 Figure 1. A Filter Paper Galvanic Cell
8. Place the red probe on Cu(s) and the black probe on Ag(s). Record the sign and value displayed.
9. Keep the red probe on Cu(s) and move the black probe to the next metal. Record the sign and value displayed.
10. While keeping the red probe on Cu(s) move the black probe to each consecutive metal. Record the sign and value for each Cu-metal combination.
11. Move the red probe to Ag(s). Keeping it on Ag(s), move the black probe around the circle making sure that you include the Cu(s) in this tour. Note: the measurements involving Al and Mg will be very unstable. Read and record the voltage value as quickly as possible after you touch the probe to the metal.
A9 KNO3 Id Figure 1. A Filter Paper Galvanic CellExplanation / Answer
QUESTION 1: Which metal is the strongest oxidizing agent in your activity table? Which metal in your table is the strongest reducing agent? Explain.
Consider the standard reduction potentials of each of the metals.
The strongest oxiding agent should have the highest reduction potential. This is beacuse it should reduce it itself, to oxidize the other species. Thus Ag is the strongest oxidizing agent.
The strongest reducing agent, oxidizes itself and reduces the other species. Therefore, it should have the lowest reduction potential. Out of this list, Mg is the strongest reducing agent.
Metal Standard Reduction Potential Mg -2.38 Al -1.66 Fe -0.04 Pb -0.13 Cu +0.34 Ag +0.80 Ni -0.25 Sn -0.14Related Questions
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