1. Given the voltaic cell shown below fill in all the blanks, a. Give the reduction and oxidation half reactions as they occur in the cell. Put an arrow in the blanks to show the direction of the movement of the cations and anions in the salt bridge. Draw an arrow to show the direction of electron movement in the wire as it passes through the voltmeter. (12 points) Given: Ni* + 2eNi (s) -0.28 eV Cd* + 2e - Cd (s) -0.40 eV Reduction reaction Oxidation reaction electron movement Salt Bridge anions cations CdSO. NISO4 (put anode/cathode labels here) b. What is the overall reaction for the electrochemical cell? (Include the phase of each component.) c. What is the potential of the cell under standard conditions? E° = d. Give the cell notation or cell diagram for the cell above. e. Which electrode is gaining mass? f. Explain the reason for the movement of cations and anions in the cell.

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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1. Given the voltaic cell shown below fill in all the blanks, a. Give the reduction and
oxidation half reactions as they occur in the cell. Put an arrow in the blanks to show the
direction of the movement of the cations and anions in the salt bridge. Draw an arrow to
show the direction of electron movement in the wire as it passes through the voltmeter.
(12 points)
Given: Ni* + 2e Ni (s) -0.28 eV
Cd* + 2e - Cd (s) -0.40 eV
Reduction reaction
Oxidation reaction
electron movement
Salt Bridge
anions
cations
CdSO.
NISO4
(put anode/cathode labels here)
b. What is the overall reaction for the electrochemical cell? (Include the phase of each
component.)
c. What is the potential of the cell under standard conditions?
E° =
d. Give the cell notation or cell diagram for the cell above.
e. Which electrode is gaining mass?
f. Explain the reason for the movement of cations and anions in the cell.
Transcribed Image Text:1. Given the voltaic cell shown below fill in all the blanks, a. Give the reduction and oxidation half reactions as they occur in the cell. Put an arrow in the blanks to show the direction of the movement of the cations and anions in the salt bridge. Draw an arrow to show the direction of electron movement in the wire as it passes through the voltmeter. (12 points) Given: Ni* + 2e Ni (s) -0.28 eV Cd* + 2e - Cd (s) -0.40 eV Reduction reaction Oxidation reaction electron movement Salt Bridge anions cations CdSO. NISO4 (put anode/cathode labels here) b. What is the overall reaction for the electrochemical cell? (Include the phase of each component.) c. What is the potential of the cell under standard conditions? E° = d. Give the cell notation or cell diagram for the cell above. e. Which electrode is gaining mass? f. Explain the reason for the movement of cations and anions in the cell.
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