What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions?E =[H+] = 0.33 MPH₂ = 3.6 atmT = 298 K

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Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 3QRT

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Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E° (V) 2H2 O(1) + 2e = H2 (g) + 20H¯ (ag) -0.83 Cu?+ (aq) + e¯ = Cu*(aq) 0.16 Cu?+ (ag) + 2e Cu(s) 0.34 O2 (g) + 4H† (aq) + 4e¯ – 2H2O(1) 1.23 Cl2 (g) + 2e 2C1¯ (aq) F2 (g) + 2e = 2F¯(aq) 1.36 2.87 Write the overall reactions that you would expect to happen when the following solutions are electrolyzed: (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. Add H,0, H*, or OH to any side of the reaction if it is needed.) a. Aqueous CuCl2. + + + b. Aqueous Cu(NO3)2. The nitrate ion is not oxidized. + + 1
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What would the potential of a standard hydrogen electrode (S.H.E.) be under the following conditions? E = [H+] = 0.33 M PH₂ = 3.6 atm T = 298 K