A. Galvanic Cells Below is the notation for each cell to be constructed. Record the highest potential reached for each cell. Zn° Zn2+(0.10 M)||Cu2+(0.10 M) |Cu° Fe° Fe2+(0.10 M)||Cu²+(0.10 M)|Cuº Yvoltage: 1.17V voltage: 0.583 V Mg0| Mg2+ (0.10 M)||Cu2+(0.10 M) |Cu° Mgº| Mg2+(0.10 M)||Zn2+(0.10 M) | Zn Zn° Zn2+(0.10 M)||Fe²+(0.10 M)| Fe° voltage: 1.522 V voltage: 0.631V Mg0| Mg2+ (0.10 M)||Fe2+ (0.10 M)| Fe° voltage: 0.527V voltage: 1.186V A. Galvanic Cells 13. Show your work using standard reduction potentials, to determine the theoreti- cal voltage for each of the combinations. Determine which half reaction occurs at the anode, and which occurs at the cathode. Also include the % error of your measurement. a. Zn° Zn2+(0.10 M)||Cu2+(0.10 M) | Cu° Anode reaction: Cathode reaction: Overall reaction: Calculated Eº: b. Fe|Fe2+ (0.10 M)||Cu2+(0.10 M)|Cu° Anode reaction: Cathode reaction: Overall reaction: Calculated E°º. c. Mg Mg2+(0.10 M)||Cu2+(0.10 M)|Cu° Anode reaction: Cathode reaction: Overall reaction: % Error: % Error: Calculated Eº. % Error:

A. Galvanic Cells Below is the notation for each cell to be constructed. Record the highest potential reached for each cell. Zn° Zn2+(0.10 M)||Cu2+(0.10 M) |Cu° Fe° Fe2+(0.10 M)||Cu²+(0.10 M)|Cuº Yvoltage: 1.17V voltage: 0.583 V Mg0| Mg2+ (0.10 M)||Cu2+(0.10 M) |Cu° Mgº| Mg2+(0.10 M)||Zn2+(0.10 M) | Zn Zn° Zn2+(0.10 M)||Fe²+(0.10 M)| Fe° voltage: 1.522 V voltage: 0.631V Mg0| Mg2+ (0.10 M)||Fe2+ (0.10 M)| Fe° voltage: 0.527V voltage: 1.186V A. Galvanic Cells 13. Show your work using standard reduction potentials, to determine the theoreti- cal voltage for each of the combinations. Determine which half reaction occurs at the anode, and which occurs at the cathode. Also include the % error of your measurement. a. Zn° Zn2+(0.10 M)||Cu2+(0.10 M) | Cu° Anode reaction: Cathode reaction: Overall reaction: Calculated Eº: b. Fe|Fe2+ (0.10 M)||Cu2+(0.10 M)|Cu° Anode reaction: Cathode reaction: Overall reaction: Calculated E°º. c. Mg Mg2+(0.10 M)||Cu2+(0.10 M)|Cu° Anode reaction: Cathode reaction: Overall reaction: % Error: % Error: Calculated Eº. % Error:

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 51QAP: For a certain cell, G=25.0 kJ. Calculate E° if n is (a) 1(b)1(c) 41 Comment on the effect that the...

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For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
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Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
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For a certain cell, G=25.0 kJ. Calculate E° if n is (a) 1(b)1(c) 41 Comment on the effect that the number of electrons exchanged has on the voltage of a cell.
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