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Use the Nernst equation to calculate the actual cell potential of a galvanic cell under the following non-standard conditions: 2 cell 1: Pt electrode 1.81 M Fe2+ 0.42 M Fe3+ 2 cell 2: Zn electrode 2.89 M Zn2+ Temperature: 30.09 °C F = 96,485.34 C/ mol e R = 8.314462J/ K-mol

Use the Nernst equation to calculate the actual cell potential of a galvanic cell under the following non-standard conditions: 2 cell 1: Pt electrode 1.81 M Fe2+ 0.42 M Fe3+ 2 cell 2: Zn electrode 2.89 M Zn2+ Temperature: 30.09 °C F = 96,485.34 C/ mol e R = 8.314462J/ K-mol

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
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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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Use the Nernst equation to calculate the actual cell potential of a galvanic cell under the following non-standard conditions: ½ cell 1: Pt electrode 1.81 M Fe2+ 0.42 M Fe3+ ½ cell 2: Zn electrode 2.89 M Zn2+ Temperature: 30.09 °C F = 96,485.34 C/ mol e %3D R = 8.314462J/ K-mol Use this Table of Standard Reduction Potentials IMPORTANT: When entering your answer: • Enter the number only (no units) • Do not leave any spaces • Include the sign if your answer is negative (not necessary for positive values) • Use a leading zero before the decimal when necessary Report your number to 2 decimal places (regardless of the significant figures) Correctly round your answer to the 2nd decimal place (there is no margin of allowed error in this question, so always use un-rounded numbers in your calculations), If the last digits
Transcribed Image Text:Use the Nernst equation to calculate the actual cell potential of a galvanic cell under the following non-standard conditions: ½ cell 1: Pt electrode 1.81 M Fe2+ 0.42 M Fe3+ ½ cell 2: Zn electrode 2.89 M Zn2+ Temperature: 30.09 °C F = 96,485.34 C/ mol e %3D R = 8.314462J/ K-mol Use this Table of Standard Reduction Potentials IMPORTANT: When entering your answer: • Enter the number only (no units) • Do not leave any spaces • Include the sign if your answer is negative (not necessary for positive values) • Use a leading zero before the decimal when necessary Report your number to 2 decimal places (regardless of the significant figures) Correctly round your answer to the 2nd decimal place (there is no margin of allowed error in this question, so always use un-rounded numbers in your calculations), If the last digits
F2 + 2 e → 2 F S,O, + 2 e → 2 SO,- Co + e → Co* MnO, + 8 H + 5 e → Mn²* + 4 H,O Au + 3 e Au (s) 2.87 2.10 1.82 1.51 1.50 C2+ 2 e → 2 CI O2 + 4 H + 4 e → 2 H½O 1.36 1.23 Br2 (1) + 2 e → 2 Br 2 Hg** + 2 e → Hg2 + 2 e → Hg) 1.07 0.92 Hg Ag Hg2* + 2 e → 2 Hg (1) Fe* + e → Fe* 0.85 e → Ag(9) 0.80 0.79 0.77 I2(6) + 2 e → 2 F Cu* + e → Cu(s) Cu+ + 2 e → Cus) 0.53 0.52 0.34 Cu* + e → Cu" 0.15 Sn** + 2 e → Sn²* S) + 2 H' + 2 e → H,S (2) 2 H* + 2 e → H2 (g) Fe + 3 e Fe) Pb 0.15 0.14 0.00 -0.04 + 2 e → Pb (s) Sn2+ + 2 e -0.13 Sn. 0 14
Transcribed Image Text:F2 + 2 e → 2 F S,O, + 2 e → 2 SO,- Co + e → Co* MnO, + 8 H + 5 e → Mn²* + 4 H,O Au + 3 e Au (s) 2.87 2.10 1.82 1.51 1.50 C2+ 2 e → 2 CI O2 + 4 H + 4 e → 2 H½O 1.36 1.23 Br2 (1) + 2 e → 2 Br 2 Hg** + 2 e → Hg2 + 2 e → Hg) 1.07 0.92 Hg Ag Hg2* + 2 e → 2 Hg (1) Fe* + e → Fe* 0.85 e → Ag(9) 0.80 0.79 0.77 I2(6) + 2 e → 2 F Cu* + e → Cu(s) Cu+ + 2 e → Cus) 0.53 0.52 0.34 Cu* + e → Cu" 0.15 Sn** + 2 e → Sn²* S) + 2 H' + 2 e → H,S (2) 2 H* + 2 e → H2 (g) Fe + 3 e Fe) Pb 0.15 0.14 0.00 -0.04 + 2 e → Pb (s) Sn2+ + 2 e -0.13 Sn. 0 14
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