A certain half-reaction has a standard reduction potential Ed=-0.37 v. An engineer proposesusing this half-reaction at the anode of a galvanic cell that must provide at least 0.60 v ofelectrical power. The cell will operate under standard conditions.Note for advanced students: assume the engineer requires this half-reaction to happen at theanode of the cell.Is there a minimum standard reductionpotential that the half-reaction used atthe cathode of this cell can have?If so, check the "yes" box and calculatethe minimum. Round your answer to 2decimal places. If there is no lowerlimit, check the "no" box.Is there a maximum standard reductionpotential that the half-reaction used atthe cathode of this cell can have?If so, check the "yes" box and calculatethe maximum. Round your answer to 2decimal places. If there is no upperlimit, check the "no" box.By using the information in the ALEKSData tab, write a balanced equationdescribing a half reaction that could beused at the cathode of this cell.Note: write the half reaction as it wouldactually occur at the cathode.O yes, there is a minimum.Ono minimum.O yes, there is a maximum.Ono maximum0Ered - Ov0Ered= OvローロeXDoallaAr

At the anode, oxidation takes place and at the cathode, reduction takes place in a galvanic cell. In…

A certain half-reaction has a standard reduction potential E -0.37 v. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 0.60 v of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at th anode of the cell. n

A certain half-reaction has a standard reduction potential E -0.37 v. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 0.60 v of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at th anode of the cell. n

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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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. 中 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? O О If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. Ον No Yes ローロ e ☐ x10 G
0 A certain half-reaction has a standard reduction potential E 'red must provide at least 0.70 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the cathode of this cell. Note: write the half reaction as it would actually occur at…
2. Tell whether each of these statements are true and false. If false, rewite it to make it a correct statement. Oxidation always occurs at the anode of an electrochemical cell. The anode of a voltaic cell is the ite of reduction and is negative. Standard conditions for electrochemical cells are a concentration of 1.0 M for disolved species and a pressure of 1 bar for gases. The potential of a voltaic cell does not change with temperature. All product-favored oxidation-reduction reactions have a standard cell voltage E°cell, with a negative sign.
Subject: chemistry
7
Element A has a standard reduction potential of +0.74V, whereas Element B has a standard reduction potential of -1.15V. Which of the following statements is correct with respect to building a Galvanic cell with these two elements? A. A will be the cathode, B will be the anode, and the cell potential will be positive. B. A will be the cathode, B will be the anode, and the cell potential will be negative. C. A will be the anode, B will be the cathode, and the cell potential will be positive. D. A will be the anode, B will be the cathode, and the cell potential will be negative. E. The anode, cathode, and cell potential must all be experimentally determined.
A certain half-reaction has a standard reduction potential E=+1.34 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.20 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer reguires this half-reaction to happen at the anode of the cell. nh Data Half-Reaction E° (V) 0.7996 Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? = Ov Ag+ (aq) + e- -→ Ag (s) O yes, there is a minimum. E %3D red Al3+ (aq) + 3e- → Al (s) -1.676 1.692 Au+ (aq) + e → Au (s) If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. O no minimum Au3+ (aq) + 3e- → Au (s) 1.498 Ba2+ (ag) + 2e- - Ba (s) -2.912 Brz (1) + 2e 2Br (aq) 1.066 - Ca2+ (ag) + 2e Ca (s) -2.868 Is there a maximum standard reduction potential that the half-reaction used at the…
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3. The Eel fora galvanic cell composed of a Li electrode and an unknown electrode was found to be 2.91 volts. Use the Standard Reduction Potential table to determine the identity of the unknown electrode. Show work. Ered (Volts) -0.80 -0.34 -0.04 -0.76 -0.14 -0.40 -2.37 Half-Reaction Ag (aq) + 1e → Ag(s) Cu²+ (aq) + 2e > Cu(s) Fe (aq) + 3e > Fe(s) Zn²+ (aq) Sn²+ (aq) + 2e +2e → Zn(s) Sn(s) Cd²+ (aq) + 2e* Cd(s) Mg²+ (aq) + 2e Mg(s)
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Consider the following galvanic cells. Diagram I Au- cº 1.0 M Au³+ 3+ chemPad XX² (b) balanced cell equation II chemPad 8⁰ XX→→ 1.0 M Cu+ 1.0 M Cu²+ For each galvanic cell, give the balanced cell reaction and determine °. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) (a) balanced cell equation I Help Greek Pt Help Greek Diagram II Cd- 1.0 M Cd2+ -Pt Ai 1.0 M VO₂, 1.0 MH+ 1.0 M VO²+
Consider the half reactions in a cell: Pb2+ + 2 e ------ Pb(s) Eo = - 0.126 V Fe3+ + e ------ Fe2+ (aq) Eo = + 0.771 V Which of the following statement is correct for the cell? Given Given A. For a Galvanic cell the standard emf will be 0.645 V and Pb will be the anode B. For a Galvanic cell standard emf will be 0.645 V and Fe will be the cathode C. For a Galvanic cell standard emf will be 1.668 V and Pb will be cathode D. For a Voltaic cell the standard emf will be 0.897 V and Fe will be the anode E. For a Voltaic cell standard emf will be 0.897 V and Pb will be the anode