A chemist designs a galvanic cell that uses these two half-reactions:MnO4(aq)+8H (aq) +SeFe³+ (aq) +eWrite a balancedequation for thehalf-reaction thathappens at thecathode.Write a balancedequation for thehalf-reaction thathappens at theanode.half-reactionWrite a balanced.equation for theAnswer the following questions about this cell.0-Mn² (aq) + 4H₂O(1)Fe (aq)standard reduction potential+1.51 VEred=+0.771 V20"red= Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction isspontaneous aswritten.Do you haveenoughinformation tocalculate the cellvoltage understandardconditions?If you said it waspossible tocalculate the cellvoltage, do so andenter your answerhere. Be sure youranswer has thecorrect number ofsignificant digits.YesNoOv

Greater the value of standard reduction potential of a redox couple , stronger be the oxidizing…

A chemist designs a galvanic cell that uses these two half-reactions: MnO (aq)+8H (aq) +5e Fe (aq)+e Write a balanced equation for the half-reaction that happens at the cathode.. half-reaction 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 0 → Mn (aq) + 4H₂O(1) Fe²(aq) 1 standard reduction potential = +1.51 V red Ed=+0.771 V red

A chemist designs a galvanic cell that uses these two half-reactions: MnO (aq)+8H (aq) +5e Fe (aq)+e Write a balanced equation for the half-reaction that happens at the cathode.. half-reaction 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 0 → Mn (aq) + 4H₂O(1) Fe²(aq) 1 standard reduction potential = +1.51 V red Ed=+0.771 V red

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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O ELECTROCHEMISTRY Designing a galvanic cell from tw... A chemist designs a galvanic cell that uses these two half-reactions: standard reduction half-reaction 2H₂O(1)+2e Write a balanced equation for the half-reaction that happens at the anode. Ered= Br₂(1)+2e Ered = +1.065 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. 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? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 3 significant digits. 0 0 0 O Yes O No H₂(g) + 2OH(aq) 2 Br (aq) V potential = -0.83 V - 3 ⠀ ローロ X 2 5 x10 S
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A student contructs an electrochemical cell consisting of a silver electrode in a 0.10 M solution of AgNO3 connected through a salt bridge to a zinc electrode in a 0.10 M solution of Zn(NO3)2. The potential across the electrochemical cell was measured as 1.52 V. a. Write the half reactions for the cathode and the anode. b. Use standard notation to represent this electrochemical cell.
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