Give the balanced cell equation and determine e° 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.) а. H2O2 + 2H+ + 2e¯→2H2O Cr2 072- + 14H+ + 6e¯ →2CR+ + 7H2O ɛ° = 1.33 V e° = 1.78 V V + + + b. + 2e →H2 La+ + 3e- -→La e° = 0.00 V ɛ° = -2.37 V 2H+ V

Give the balanced cell equation and determine e° 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.) а. H2O2 + 2H+ + 2e¯→2H2O Cr2 072- + 14H+ + 6e¯ →2CR+ + 7H2O ɛ° = 1.33 V e° = 1.78 V V + + + b. + 2e →H2 La+ + 3e- -→La e° = 0.00 V ɛ° = -2.37 V 2H+ V

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the standard potential...

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Give the balanced cell equation and determine e° 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.)
а.
H2O2 + 2H+ + 2e¯→ 2H20
ɛ° = 1.78 V
Cr2 O7
+ 14H+ + 6e →2 Cr³+
+ 7H2O ɛ° = 1.33 V
V
+
+
+
b.
2H+ + 2e →H2 ɛ° = 0.00 V
La3+ + Зe —La
-2.37 V
V
+
+

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