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Question 5, Part d: How much energy (in kJ) can be derived from the oxidation of 6.75 g of aluminum at an average cell potential of 2.00 V?

Question 5, Part d: How much energy (in kJ) can be derived from the oxidation of 6.75 g of aluminum at an average cell potential of 2.00 V?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question 5, Part d:

How much energy (in kJ) can be derived
from the oxidation of 6.75 g of aluminum at an average cell potential of 2.00 V?
**5. Consider the following standard reduction (half-cell) potentials:** \[ \text{Al}^{3+} (\text{aq}) + 3e^- \rightarrow \text{Al} (\text{s}); \quad E^\circ = -1.66 \, \text{V} \] \[ \text{Cu}^{2+} (\text{aq}) + 2e^- \rightarrow \text{Cu} (\text{s}); \quad E^\circ = +0.34 \, \text{V} \] (a) Sketch a voltaic cell consisting of the above half-cells using KNO\(_3\) as a salt-bridge. Label the following: (i) the anode and cathode half-cells; (ii) the positive and negative electrodes; (iii) the direction electron flows in the circuit and ions flow in the salt bridge. (b) Write the net equation for the overall cell reaction and calculate the standard cell potential (E\(_\text{cell}^\circ\)) at 25°C. (c) Calculate ΔG° for the overall reaction at 25 °C. (d) How much energy (in kJ) can be derived from the oxidation of 6.75 g of aluminum at an average cell potential of 2.00 V?
Transcribed Image Text:**5. Consider the following standard reduction (half-cell) potentials:** \[ \text{Al}^{3+} (\text{aq}) + 3e^- \rightarrow \text{Al} (\text{s}); \quad E^\circ = -1.66 \, \text{V} \] \[ \text{Cu}^{2+} (\text{aq}) + 2e^- \rightarrow \text{Cu} (\text{s}); \quad E^\circ = +0.34 \, \text{V} \] (a) Sketch a voltaic cell consisting of the above half-cells using KNO\(_3\) as a salt-bridge. Label the following: (i) the anode and cathode half-cells; (ii) the positive and negative electrodes; (iii) the direction electron flows in the circuit and ions flow in the salt bridge. (b) Write the net equation for the overall cell reaction and calculate the standard cell potential (E\(_\text{cell}^\circ\)) at 25°C. (c) Calculate ΔG° for the overall reaction at 25 °C. (d) How much energy (in kJ) can be derived from the oxidation of 6.75 g of aluminum at an average cell potential of 2.00 V?
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