A chemist designs a galvanic cell that uses these two half-reactions:standard reduction potentialExedhalf-reaction2 H2O(1)+2e→H2(g)+2OH (aq)Εred-0.83 V2+Zn(aq)+2e→>>Zn(s)E= = -0.763 V'redAnswer the following questions about this cell. Write a balancedequation for thehalf-reaction thathappens at thecathode.Write a balancedequation for thehalf-reaction thathappens at theanode.Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction isspontaneous aswritten.Do you haveenoughinformation tocalculate the cellvoltage understandardconditions?☐☐☐оYesONoIf you said it waspossible tocalculate the cellvoltage, do so andenter your answerhere. Round youranswer to 1significant digit.Ovローロе

Answered: Image /qna-images/answer/fea0740c-aa65-4954-baf6-9250529e30b2.jpg

Answered: A chemist designs a galvanic cell that…

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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Consider a galvanic electrochemical cell constructed using Cr/Cr** and Zn/Zn2* at 25 °C. The following half-reactions are provided for each metal: 3+ Cr**(aq) + 3 e → Cr(s) E°red = -0.744 V Zn2*(aq) + 2 e → Zn(s) E°red = -0.763 V What is the cell potential for this cell at 25 °C when [Zn2*] = 0.0323 M and [Cr3] = 0.1736 M?
Use the standard reduction potentials given below to predict if a reaction will occur between Co(s) and I₂ (s), when the two are brought in contact via standard half-cells in a voltaic cell. I2 (s) + 2e → 21¯ (aq) Eº = 0.535 V red Co²+ (aq) + 2e → Co(s) Ee = -0.280 V red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (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 chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Zn"(aq)+2e Zn(s) E=-0.763 V "red MnO,(s)+4H (aq)+2e¯ - Mn²"(aq)+2H,0m E=+1.23 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that U happens at the cathode. O OP Write a balanced equation for the half-reaction that happens at the anode. ? Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? Yes O No If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 3 significant digits.
Suppose the galvanic cell sketched below is powered by the following reaction: Mn(s)+ FeCl,(aq) → MnCl,(aq)+Fe(s) e- E1 E2 S1 S2
A galvanic cell is powered by the following redox reaction: 2+ 2 Zn²+(aq) + N₂H₂(aq) + 4OH¯(aq) → 2 Zn(s) + N₂(g) + 4H₂O(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 0 0 E = V 00 S
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Consider a galvanic cell based on the following half reactions: E (V) M4+ + 4e M 0.66 N3+ ++3e N 0.10 Assuming the value of Faraday's constant is 96,485 C/mol e, the value of AG° for this cell is J
A galvanic cell is powered by the following redox reaction: Br,(1) + H,(g) + 2 OH (aq) - 2 Br (aq) + 2 H,O(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. O-0 Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. E = [y Round your answer to 2 decimal places. Explanation Check O 2022 McGraw Hill LLC. All Riahts Reserved. Terms of Use F étv 17
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction Br₂(1)+2e → 2 Br (aq) N₂(g) + 4H₂O()+4e N₂H₂(aq)+4 OH (aq) standard reduction potential E 'red E = red +1.065 V - 1.16 V
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2 H₂O(1)+2e →> H2(g)+2 OH (aq) E.ed = -0.83 V red Cu²+(aq)+e Cu+ (aq) →>> Answer the following questions about this cell. E° = +0.153 V red 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. Write a balanced equation for the ☐ ☐
Use the standard reduction potentials given below to predict if a reaction will occur between Ag(s) and F2 (g), when the two are brought in contact via standard half-cells in a voltaic cell. F2 (g)+2e7 →2F (aq) E red Agt (ag)+e → Ag(s) E red + = If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) - 2.870 V 0.799 V +
Could you please solve the last two questions from the second picture?

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