A chemist designs a galvanic cell that uses these two half-reactions:MnO4(aq) + 2 H₂O(1)+3eWrite a balancedequation for thehalf-reaction thathappens at thecathode.Write a balancedequation for thehalf-reaction that 0happens at theanode.Write a balanced.equation for theoverall reactionthat powers thecell. Be sure thereaction isspontaneous aswritten.Do you haveenoughAnswer the following questions about this cell.information tocalculate the cellvoltage under*standardconditions?half-reactionIf you said it waspossible tocalculate the cellvoltage, do so andZn²+ (aq) + 2eenter your answerhere. Round youranswer to 3significant digits.O Ye's1O NoOvMnO2(s)+4OH(aq)Zn(s)standard reduction potentialE'redEred=-0.763 V= = +0.59 VeX00

Answered: Image /qna-images/answer/1e96b81f-192a-4729-b3a2-2df278e33810.jpg

A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq) + 2 H₂O(1)+3e Zn²+ (aq) + 2e Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that O happens at the anode. Write a balanced- equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Answer the following questions about this cell. Do you have enough information to calculate the cell voltage under standard conditions? half-reaction If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 3 O Yes - O No MnO₂ (s) + 4 OH (aq) → Zn(s) standard reduction potential E=+0.59 V "red . . Ed=-0.763 V red 3-0 X 2 0 0²

A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq) + 2 H₂O(1)+3e Zn²+ (aq) + 2e Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that O happens at the anode. Write a balanced- equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Answer the following questions about this cell. Do you have enough information to calculate the cell voltage under standard conditions? half-reaction If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 3 O Yes - O No MnO₂ (s) + 4 OH (aq) → Zn(s) standard reduction potential E=+0.59 V "red . . Ed=-0.763 V red 3-0 X 2 0 0²

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A galvanic cell is powered by the following redox reaction: 3 Br₂(1) + 2NO(g) + 4H₂O(1) - 6 Br (aq) + 2NO3(aq) + 8H (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 0 E = v 00 Ś
A galvanic cell is powered by the following redox reaction: Cl₂(g) + 2NO(g) + 2 H₂O(1) → 2 CI (aq) + 2 HNO₂(aq) + 2H¹ (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. E = v ローロ e
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A galvanic cell is powered by the following redox reaction: 2+ MnO₂ (s) + 4H* (aq) + 2 Br¯ (aq) → Mn²(aq) + 2 H₂O(1) + Br₂(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 = = Ov ローロ 0
A chemist designs a galvanic cell that uses these two half-reactions: 2 H₂O(1)+2e 2+ Zn² (aq) +2e Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Answer the following questions about this cell. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough half-reaction information to calculate the cell voltage under standard conditions? significant digit 0 0 Yes No If you said it was possible to calculate the cell voltage, do so and enter your answer ☐V here. Round your answer to 1 H₂(g) + 2 OH (aq) Zn(s) standard reduction potential Eº red Eve 'red 0.83 V == - 0.763 V ロ→ロ X 90 x10
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A galvanic cell is powered by the following redox reaction: 2+ 2 Cu²+ (aq) + H₂(g) + 2OH¯(aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 □ 0 E = v + 2 Cu (aq) + 2 H₂O(1) ロ→ X Ś
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