L. Balance the following Galvanic cell redox reactions and write its cell notation.1. 2Cro) + 3Cu*(aq)2Cr (aq) +3Cu()2. 5Fe*(aq) + Mno, (aq) + 8H (aq)- SFe (aq) + Mn (aq) + 4H,O()

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Answered: L. Balance the following Galvanic cell…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter18: Oxidation–reduction Reactions And Electrochemistry

Section: Chapter Questions

Problem 28A

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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?
For a voltage-sensitive application, you are working on a battery that must have a working voltage of 0.85 V. The half-cells to be used have a standard cell potential of 0.97 V. What must be done to achieve the correct voltage? What information would you need to look up?
Give the notation for a voltaic cell whose overall cell reaction is Mg(s)+2Ag+(aq)Mg2+(aq)+2Ag(s) What are the half-cell reactions? Label them as anode or cathode reactions. What is the standard cell potential of this cell?
At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.
For the following half-reactions, answer these questions. Ce4+(aq)+eCe3+(aq)E=+1.61VAg+(aq)+eAg(s)E=+0.80VHg22+(aq)+2e2Hg(l)E=+0.80VSn2+(aq)+2eSn(s)E=0.14VNi2+(aq)+2eNi(s)E=0.24VAl3+(aq)+3eAl(s)E=1.68V (a) Which is the weakest oxidizing agent? (b) Which is the strongest oxidizing agent? (c) Which is the strongest reducing agent? (d) Which is the weakest reducing agent? (e) Will Sn(s) reduce Ag+(aq) to Ag(s)? (f) Will Hg(l) reduce Sn2+(aq) to Sn(s)? (g) Which ion(s) can be reduced by Sn(s)? (h) Which metal(s) can be oxidized by Ag+(aq)?
A voltaic cell is constructed using the reaction Mg(s) + 2H+(aq) Mg2+(aq) + H2(g) (a) Write equations for the oxidation and reduction half-reactions. (b) Which half-reaction occurs in the anode compartment, and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the ________ electrode to the ______ electrode. Negative ions move in the salt bridge from the ______ half-cell to the ______ half-cell. The half-reaction at the anode is ____, and that at the cathode is _____.
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
The following oxidationreduction reactions are used in electrochemical cells. Write them using cell notation. (a) 2Ag+(aq)(0.50M)+Ni(s)2Ag(s)+Ni2+(aq)(0.20M) (b) Cu(s)+PtCl62-(aq)(0.10M)Cu2+(aq)(0.20M)+PtCl42-(aq)(0.10M)+2Cl(aq)(0.40M) (c) Pb(s)+SO42-(aq)(0.30M)+2AgCl(s)PbSO4(s)+2Ag(s)+2Cl(aq)(0.20M) (d) In a galvanic cell, one half-cell contains 0.010 M HCI and a platinum electrode, over which H2 is bubbled at a pressure of 1.0 atm. The other half-cell is composed of a zinc electrode in a 0.125 M solution of Zn(NO3)2.
The standard potential for the reduction of AgSCN is 0.0895 V. AgSCN(s)+eAg(s)+SCN(aq) Find another electrode potential to use together with the above value and calculate Kspfor AgSCN.
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the following questions. Give reasons for your answers. (Use data from Table 17-1.) a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by SO42 (aq) in acid? d. Which species can be reduced by Al(s)?
A solution contains the ions H+, Ag+, Pb2+, and Ba2+, each at a concentration of 1.0 M. (a) Which of these ions would be reduced first at the cathode during an electrolysis? (b) After the first ion has been completely removed by electrolysis, which is the second ion to be reduced? (c) Which, if any, of these ions cannot be reduced by the electrolysis of the aqueous solution?

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L. Balance the following Galvanic cell redox reactions and write its cell notation. 1. 2Cr) + 3Cu" (aq) 20 (aq) + 3Cu(o) 2. 5Fe*(aq) + Mno, (aq) + 8H (ag)- SFe (aq) + Mn*(aq) + 4H,O()

L. Balance the following Galvanic cell redox reactions and write its cell notation. 1. 2Cr) + 3Cu" (aq) 20 (aq) + 3Cu(o) 2. 5Fe(aq) + Mno, (aq) + 8H (ag)- SFe (aq) + Mn(aq) + 4H,O()