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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.) a. H₂O2 + 2H+ + 2e¯ → 2H₂O € = 1.78 V 2- Cr₂O7²- + 14H+ + 6e¯ →2 Cr³+ + 7H₂O €° = 1.33 V V + b. 2H+ + 2e →H₂ La³+ + 3e¯→La €° = V + + + = 0.00 V ɛ° = −2.37 V +

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.) a. H₂O2 + 2H+ + 2e¯ → 2H₂O € = 1.78 V 2- Cr₂O7²- + 14H+ + 6e¯ →2 Cr³+ + 7H₂O €° = 1.33 V V + b. 2H+ + 2e →H₂ La³+ + 3e¯→La €° = V + + + = 0.00 V ɛ° = −2.37 V +

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
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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Give the balanced cell equation and determine ɛ° 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 € 2- O Cr₂O7²- + 14H+ + 6e¯ →2 Cr³+ + 7H₂O €° = V a. €° + + b. 2H+ + 2e →H₂ La³+ + 3e¯ →La ɛ° 2.3+ ɛ° = V + E + O + = 0.00 V = -2.37 V = 1.78 V 1.33 V
Transcribed Image Text:Give the balanced cell equation and determine ɛ° 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 € 2- O Cr₂O7²- + 14H+ + 6e¯ →2 Cr³+ + 7H₂O €° = V a. €° + + b. 2H+ + 2e →H₂ La³+ + 3e¯ →La ɛ° 2.3+ ɛ° = V + E + O + = 0.00 V = -2.37 V = 1.78 V 1.33 V
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