Give the balanced cell equation and determine & for the galvanic cells based on the following half-reactions. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) H₂O2 + 2H+ + 2e → 2H₂O Cr₂O72- + 14H+ + 6e €° = a. b. € V 2H+ + 2e → H₂ A1³+ + 3e → Al = + V + € = 1.78 V 2 Cr³+ + 7H₂O = 1.33 V € = 0.00 V E = -1.66 V +

Chemistry: Principles and Practice
3rd Edition
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Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.46QE
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Give
the balanced cell equation and determine & for the galvanic cells based on the following half-reactions.
(Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)
H₂O2 + 2H+ + 2e → 2H₂O
€ = 1.78 V
Cr₂O7²- + 14H+ + 6e¯ →2 Cr³+ + 7H₂O €° = 1.33 V
a.
b.
€ =
V
€ =
+
2H+ + 2e → H₂
→ Al
A1³+ +3e
V
€ = 0.00 V
€ = -1.66 V
Transcribed Image Text:Give the balanced cell equation and determine & for the galvanic cells based on the following half-reactions. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) H₂O2 + 2H+ + 2e → 2H₂O € = 1.78 V Cr₂O7²- + 14H+ + 6e¯ →2 Cr³+ + 7H₂O €° = 1.33 V a. b. € = V € = + 2H+ + 2e → H₂ → Al A1³+ +3e V € = 0.00 V € = -1.66 V
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