half-cell and aare 0.0530 MMISSED THIS? Read Section 20.6 (Page).A voltaic cell consists of a Pb/Pb²+Cu/Cu²+ half-cell at 25 °C. The initialconcentrations of Pb²+and Cu²+2+and 1.70 M, respectively.What is the initial cell potential?Express your answer using two significant figures.►View Available Hint(s)IVE ΑΣΦEcell:=SubmitPart B2+What is the cell potential when the concentration of CuExpress your answer using two significant figures.► View Available Hint(s)[5] ΑΣΦEcell ==SubmitPart C?Vhas fallen to 0.250 M??VWhat is the concentration of Pb²+ when the cell potential falls to 0.350 V ?Express your answers using three significant figures.►View Available Hint(s)

The given cell is a voltaic cell consisting of Pb/Pb2+ and Cu/Cu2+. A voltaic cell is an…

MISSED THIS? Read Section 20.6 (Page). A voltaic cell consists of a Pb/Pb²+ half-cell and a Cu/Cu²+ half-cell at 25 °C. The initial concentrations of Pb2+ and Cu²+ are 0.0530 M and 1.70 M, respectively. What is the initial cell potential? Express your answer using two significant figures. View Available Hint(s) 15| ΑΣΦ Ecell = Submit Part B Ecell = What is the cell potential when the concentration of Cu²+ has fallen to 0.250 M? Express your answer using two significant figures. View Available Hint(s) Submit Part C ? [5] ΑΣΦ V ? V What is the concentration of Pb2+ when the cell potential falls to 0.350 V ? Express your answers using three significant figures

MISSED THIS? Read Section 20.6 (Page). A voltaic cell consists of a Pb/Pb²+ half-cell and a Cu/Cu²+ half-cell at 25 °C. The initial concentrations of Pb2+ and Cu²+ are 0.0530 M and 1.70 M, respectively. What is the initial cell potential? Express your answer using two significant figures. View Available Hint(s) 15| ΑΣΦ Ecell = Submit Part B Ecell = What is the cell potential when the concentration of Cu²+ has fallen to 0.250 M? Express your answer using two significant figures. View Available Hint(s) Submit Part C ? [5] ΑΣΦ V ? V What is the concentration of Pb2+ when the cell potential falls to 0.350 V ? Express your answers using three significant figures

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

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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 standard potential for this cell? b. A nonstandard cell is set up at 25C with [Mg2+] = 1.00 105 M. The cell potential is observed to be 4.01 V. Calculate [Au3+] in this cell.
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 the cell described below: Zn|Zn2+(1.00M)||Cu2+(l.00M)|Cu Calculate the cell potential after the reaction has operated long enough for the [Zn2+] to have changed by 0.20 mol/L. (Assume T=25C.)
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
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?
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?
What is the standard cell potential you would obtain from a cell at 25C using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?
For the standard cell potentials given here, determine the ?G for the cell in k].. (a) 0.000V,n=2 (b) +0.434V,n=2 (c) -2.439 V, n = 1
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4] = 0.010 M, [Br] = 0.010 M. [Mn2] = 0.15 M, and [H] = 1.0 M. 2MNO4(aq)+10Br(aq)+16H+(aq)2MN2(aq)+5Br2(l)+8H2O(l)
Calculate the standard cell potential of the following cell at 25C. Sn(s)Sn2+(aq)I2(aq)I(aq)

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