Reduction potentials 1. The first voltage you measure is negative. What should y

Question

Reduction potentials 1. The first voltage you measure is negative. What should you do?
2. You are unable to measure a voltage between any of the metals in the experiment. The voltmeter is properly functioning, and the metals are correctly connected. Suggest an explanation.
3. What do you expect the cell potential to be for the following redox couples with oxidation states of zero and +2: a. Cu and Fe b. Fe and Zn c. Zn and Cu Reduction potentials 1. The first voltage you measure is negative. What should you do?
2. You are unable to measure a voltage between any of the metals in the experiment. The voltmeter is properly functioning, and the metals are correctly connected. Suggest an explanation.
3. What do you expect the cell potential to be for the following redox couples with oxidation states of zero and +2: a. Cu and Fe b. Fe and Zn c. Zn and Cu Reduction potentials 1. The first voltage you measure is negative. What should you do?
2. You are unable to measure a voltage between any of the metals in the experiment. The voltmeter is properly functioning, and the metals are correctly connected. Suggest an explanation.
3. What do you expect the cell potential to be for the following redox couples with oxidation states of zero and +2: a. Cu and Fe b. Fe and Zn c. Zn and Cu

Explanation / Answer

1.A voltage itself has no sign, without a reference. You can change the position of the wires that connect the voltmeter to the measured circuit to obtain a positive value/change the sign.

2.You don’t have a solution in the eletrochemical cell.

3. Look to a Table of standard reduction potentials;

a. 0.521 – ( -0.44) = 0.96 V

b. -0.44 – (-0.76) = 0.32 V

c. 0.521 – (-0.76) = 1.28 V

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