2 For the following electrochemical cell, which of the following statementsis truewhen the cell operates spontaneously? (That is, when e are allowed toflowwhichever way they "want" to)?Pt(s)Cu(s)1 M CIO, (aq)1 M CIO, (aq)1MH (aq)1 M Cu*(aq)O voltage = .148 V; electrons move from right to left (<---)%3DO voltage = 1.71 V; electrons move from right to left (<---)O voltage = .669 V; electrons move from right to left (<---)%3!O voltage = 1.71 V; electrons move from left to right (--->)%3DO voltage = .669 V; electrons move from left to right (--->)%3DIf a chemical reaction has AG°298= +31.9 kJ, what is the equilibriumconstantKeg at 298 K?O 2.6 x 106O 3.9 x 105O 12.90 1.3х 1013O 7.5 x 1012

1.) From given cell , firat we would write possible half reactions as per given compounds and…

For the following electrochemical cell, which of the following statements is true when the cell operates spontaneously? (That is, when e are allowed to flow whichever way they "want" to)? Pt(s) Cu(s) 1 M CIO, (aq) 1 M CIO, (aq) 1 MH (aq) 1 M Cu*(aq) O voltage = .148 V; electrons move from right to left (<---) %3D O voltage = 1.71 V; electrons move from right to left (<--) %3D O voltage = .669 V; electrons move from right to left (<---) %3D voltage = 1.71 V; electrons move from left to right (-->) %3D o voltage = .669 V; electrons move from left to right (--->) %3D If a chemical reaction has AG°298= +31.9 kJ, what is the equilibrium constant Keg at 298 K? O 2.6 x 106 O 3.9 x 105 O 12.9 1.3 x 10 13 O 7.5 x 1012

For the following electrochemical cell, which of the following statements is true when the cell operates spontaneously? (That is, when e are allowed to flow whichever way they "want" to)? Pt(s) Cu(s) 1 M CIO, (aq) 1 M CIO, (aq) 1 MH (aq) 1 M Cu*(aq) O voltage = .148 V; electrons move from right to left (<---) %3D O voltage = 1.71 V; electrons move from right to left (<--) %3D O voltage = .669 V; electrons move from right to left (<---) %3D voltage = 1.71 V; electrons move from left to right (-->) %3D o voltage = .669 V; electrons move from left to right (--->) %3D If a chemical reaction has AG°298= +31.9 kJ, what is the equilibrium constant Keg at 298 K? O 2.6 x 106 O 3.9 x 105 O 12.9 1.3 x 10 13 O 7.5 x 1012

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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Similar questions

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)
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?
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?
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 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 half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
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.
A lead storage battery delivers a current of 6.00 A for one hour and 22 minutes at a voltage of 12.0 V. (a) How many grams of lead are converted to PbSO4? (b) How much electrical energy is produced in kilowatt hours?
You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.

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