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QUESTION 3 Calculate the equilibrium constant for the following redox reaction at 298K, using the table provided: Express your answer to one significant figure and express your answer in scientific notation. 3F22+(aq) + 2Cr(s) → 3Fe(s) + 2Cr³*(aq) Electrochemical Potentials Half reaction E° (V) Cr3*(aq) + 3e →Cr(s) - 0.740 Cu2*(aq + Cu*(aq) + 0.153 Fe2*(aq) + 2e™ Fe(s) 0.440 Sn4+(aq) + 2e → Sn2*(aq) + 0.154 Zn2+(aq) + 2e → Zn(s) 0.763

QUESTION 3 Calculate the equilibrium constant for the following redox reaction at 298K, using the table provided: Express your answer to one significant figure and express your answer in scientific notation. 3F22+(aq) + 2Cr(s) → 3Fe(s) + 2Cr³*(aq) Electrochemical Potentials Half reaction E° (V) Cr3*(aq) + 3e →Cr(s) - 0.740 Cu2*(aq + Cu*(aq) + 0.153 Fe2*(aq) + 2e™ Fe(s) 0.440 Sn4+(aq) + 2e → Sn2*(aq) + 0.154 Zn2+(aq) + 2e → Zn(s) 0.763

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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QUESTION 3 Calculate the equilibrium constant for the following redox reaction at 298K, using the table provided: Express your answer to one significant figure and express your answer in scientific notation. 3FE2+(aq) + 2Cr(s) → 3Fe(s) +2Cr³*(aq) Electrochemical Potentials Half reaction E° (V) Cr3*(aq) + 3e →Cr(s) - 0.740 Cu2+(aq) + Cu*(aq) + 0.153 Fe2*(aq) + 2e¯ → Fe(s) - 0.440 Sn4+(aq) + 2e Sn2*(aq) + 0.154 Zn2*(aq) + 2e Zn(s) - 0.763
Transcribed Image Text:QUESTION 3 Calculate the equilibrium constant for the following redox reaction at 298K, using the table provided: Express your answer to one significant figure and express your answer in scientific notation. 3FE2+(aq) + 2Cr(s) → 3Fe(s) +2Cr³*(aq) Electrochemical Potentials Half reaction E° (V) Cr3*(aq) + 3e →Cr(s) - 0.740 Cu2+(aq) + Cu*(aq) + 0.153 Fe2*(aq) + 2e¯ → Fe(s) - 0.440 Sn4+(aq) + 2e Sn2*(aq) + 0.154 Zn2*(aq) + 2e Zn(s) - 0.763
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