QUESTION 5 Consider the following standard reduction half-reactions: A3+ (aq) +3 e-Al (s) E' = -1.66 V Ni2+ (aq) +2 e-Ni (s) E' = -0.28 V What is the cell potential when the two half-reactions above are combined to form a voltaic cell if the concentration of N2 is 4. and the concentration of A3+ is 0.000024 M? Report your answer to two decimal places.

QUESTION 5 Consider the following standard reduction half-reactions: A3+ (aq) +3 e-Al (s) E' = -1.66 V Ni2+ (aq) +2 e-Ni (s) E' = -0.28 V What is the cell potential when the two half-reactions above are combined to form a voltaic cell if the concentration of N2 is 4. and the concentration of A3+ is 0.000024 M? Report your answer to two decimal places.

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 105QAP: Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a)...

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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?
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
A solution containing a metal ion (M2+(aq)) is electrolyzed by a current of 7.8 A. After 15.5 minutes, 2.39 g of the metal is plated out. (a) How many coulombs are supplied by the battery? (b) What is the metal? (Assume 100% efficiency.)
Calculate E° for the following voltaic cells: (a) 2Na(s)+Fe2+(aq)2Na+(aq)+Fe(s) (b) 3SO42(aq)+12H+(aq)+2Al(s)3SO2(g)+2Al3+(aq)+6H2O (c) 2S(s)+4OH(aq)O2(g)+2S2(aq)+2H2O (basic)
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
Calculate the theoretical potential of each of the following cells.Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Bi|BiO+ (0.0300 M),H+ (0.100 M)||I- (0.100 M), AgI(sat’d)|Ag (b) Zn|Zn2+(5.75 10-4M)||Fe(CN)64-(530 10-2 M),Fe(CN)63-(6.75 10-2M)|Pt (c) Pt,H2O (0.200 atm)|HCI(8.25 10-4M), AgCI(sat’d)| Ag
In biological systems, acetate ion is converted to ethyl alcohol in a two-step process: CH3COO(aq)+3H+(aq)+2eCH3CHO(aq)+H2OE=0.581V CH3CHO(aq)+2H+(aq)+2eC2H5OH(aq)E=0.197V (E°' is the standard reduction voltage at 25°C and pH of 7.00.) (a) Calculate G°' for each step and for the overall conversion. (b) Calculate E°' for the overall conversion.
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?
Which of the changes below will increase the voltage of the following cell? Co|Co2+(0.010M)H+(0.010M)|H2(0.500atm)|Pt (a) Increase the volume of COCl2 solution from 100 mL to 300 mL. (b) Increase [H+] from 0.010 M to 0.500 M. (c) Increase the pressure of H2 from 0.500 atm to 1 atm. (d) Increase the mass of the Co electrode from 15 g to 25 g. (e) Increase [CO2+] from 0.010 M to 0.500 M.
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25C if the copper electrode is placed in a solution in which [Cu2+] = 2.5 104 M? b. The copper electrode is placed in a solution of unknown [Cu2+]. The measured potential at 25C is 0.195 V. What is [Cu2+]? (Assume Cu2+ is reduced.)
Consider a voltaic cell in which the following reaction takes place. 2F2+(aq)+H2O2(aq)+2H+(aq)2Fe3+(aq)+2H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Calculate E at 25°C under the following conditions: [Fe2+]=0.00813M,[H2O2]=0.914M,[Fe3+]=0.199M,ph=2.88 .
Sketch a galvanic cell, and explain how it works. Look at Figs. 17-1 and 17-2. Explain what is occurring in each container and why the cell in Fig. 17-2 works but the one in Fig. 17-1 does not.