Assume that you want to construct a voltaic cell that uses the foilowing half rea A2*(aq) + 2 e →A(s) B2*(aq) + 2 e→ B(s) E° =-0.10 V E° = -1.10 V %3D You begin with the incomplete cell pictured. a. What addition must you make to the cell to generate a standard voltage? b. What voltage will the cell generate under standard conditions? c. Which electrode is the cathode? с. pe o buens exog phpo d. Which direction will the electrons flow?

Assume that you want to construct a voltaic cell that uses the foilowing half rea A2(aq) + 2 e →A(s) B2(aq) + 2 e→ B(s) E° =-0.10 V E° = -1.10 V %3D You begin with the incomplete cell pictured. a. What addition must you make to the cell to generate a standard voltage? b. What voltage will the cell generate under standard conditions? c. Which electrode is the cathode? с. pe o buens exog phpo d. Which direction will the electrons flow?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 115AE: The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making...

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Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
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?
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
Consider the voltaic cell 2 Ag+(aq) + Cd(s) 2 Ag(s) + Cd2+(aq) operating at 298 K. (a) Calculate the Ecell for this cell. (b) If (cone. Cd2+) = 2.0 M and (cone. Ag+) = 0.25 M, calculate Ecell. (c) If Ecell = 1.25 V and (cone. Cd2+) = 0.100 M, calculate(cone. Ag+).
Consider a battery made from one half-cell that consists of a capper electrode in 1 M CuSO4 solution and another half—cell that consists of a lead electrode in 1 M Pb(NO3)2 solution. (a) What are the reactions at the anode, cathode, and the overall reaction? (b) What is the standard cell potential for the battery? (c) Most devices designed to use dry-cell batteries can operate between 1.0 and 1.5 V. Could this tell he used to make a battery that could replace a dry-cell battery? Why or why not. (d) Suppose sulfuric acid is added to the half—cell with the lead electrode and some PbSO4(s) forms. Would the cell potential increase, decrease, or remain the same?
Calculate E° for the following voltaic cells: (a) MnO2+4H+(aq)+2I(aq)Mn2+(aq)+2H2O+I2(s) (b) H2(g)+2OH(aq)+S(s)2H2O+S2(aq) (c) an Ag-Ag+ half-cell and an Au-AuCl4- half-cell
Why is a salt bridge necessary in galvanic cells like the one in Figure 17.4?
A metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
The following half-cells are available: (i) Ag+(aq, 1.0M)|Ag(s) (ii) Zn2+(aq, 1.0 M) |Zn(s) (iii) Cu2+(aq, 1.0M)|Cu(s) (iv) Co2+(aq, 1.0M)|Co(s) Linking any two half-cells makes a voltaic cell. Given four different half-cells, six voltaic cells are possible. These are labeled, for simplicity, Ag-Zn, Ag-Cu, Ag-Co, Zn-Cu, Zn-Co, and Cu-Co. (a) In which of the voltaic cells does the copper electrode serve as the cathode? In which of the voltaic cells does the cobalt electrode serve as the anode? (b) Which combination of half-cells generates the highest potential? Which combination generates the lowest potential?
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
Two Ag+(aq) | Ag(s) half-cells are constructed. The first has [Ag+] = 1.0 M, the second has [Ag+] = 1.0 105 M. When linked together with a salt bridge and external circuit, a cell potential is observed. (This kind of voltaic cell is referred to as a concentration cell.) (a) Draw a picture of this cell, labeling all components. Indicate the cathode and the anode, and indicate in which direction electrons flow in the external circuit. (b) Calculate the cell potential at 298 K.