The Sher expert Hand written solution is not allowed please QUESTION 6A voltaic cell is prepared using copper and silver. Its cell notation is shown below.Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s)Which of the following processes occurs at the cathode?Cu(s) → Cu2+(aq) + 2e¯Cu2+(aq) +A)B)+2e → → Cu(s)C)Ag(s) Ag+(aq) + e¯D)Ag+(aq) + e Ag(s)E)Cu(s) + 2Ag+(aq) → Cu²+(aq) + 2Ag(s)→

Option a: This option is incorrect because it shows the oxidation half reaction. Option b: This…

Answered: QUESTION 6 A voltaic cell is prepared…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 93QRT

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Consider a cell based on the following half-reactions: a. Draw this cell under standard conditions, labeling the anode, the cathode, the direction of electron flow, and the concentrations, as appropriate. b. When enough NaCl(s) is added to the compartment containing gold to make the [Cl] = 0.10 M, the cell potential is observed to be 0.31 V. Assume that Au3+ is reduced and assume that the reaction in the compartment containing gold is Au3+(aq)+4Cl(aq)AuCl4(aq) Calculate the value of K for this reaction at 25C.
A voltaic cell is constructed using the reaction of chromium metal and iron(II) ions. 2 Cr(s) + 3 Fe2+(aq) 2 Cr3+(aq) + 3 Fe(s) 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 ________.
A voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous solution of AgNO3.The other half cell consists of an inert platinum wire in an aqueous solution containing Fe2+(aq) and Fe3+(aq). (a) Calculate the cell potential, assuming standard conditions. (b) Write the net ionic equation for the reaction occurring in the cell. (c) Which electrode is the anode and which is the cathode? (d) If [Ag+] is 0.10 M, and [Fe2+] and [Fe3+] are both 1.0 M, what is the cell potential? Is the net cell reaction still that used in part (a)? If not, what is the net reaction under the new conditions?
Consider the following cell running under standard conditions: Fe(s)Fe2+(aq)Al3+(aq)Al(s) a Is this a voltaic cell? b Which species is being reduced during the chemical reaction? c Which species is the oxidizing agent? d What happens to the concentration of Fe3+(aq) as the reaction proceeds? e How does the mass of Al(s) change as the reaction proceeds?
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 the following galvanic cell: Calculate the concentrations of Ag+(aq) and Ni2+(aq) once the cell is dead.
The voltaic cell is represented as Zn(s)Zn2+(1.0M)Cu2+(1.0M)Cu(s) Which of the following statements is not true of this cell? a The mass of the zinc electrode, Zn(s), decreases as the cell runs. b The copper electrode is the anode. c Electrons flow through the external circuit from the zinc electrode to the copper electrode. d Reduction occurs at the copper electrode as the cell runs. e The concentration of Cu2+ decreases as the cell runs.
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)?
In principle, a battery could be made from aluminum metal and chlorine gas. (a) Write a balanced equation for the reaction thatwould occur in a battery using Al3+(aq) | Al(s) andCl2(g) | Cl(aq) half-cells. (b) Identify the half-reaction at the anode and at the cathode. Do electrons flow from the Al electrode when thecell does work? Explain. (c) Calculate the standard potential, Ecell, for the battery.
The zinc copper voltaic cell shown with this problem is currently running under standard conditions. How would the intensity of light from the bulb change if you were to a dissolve some additional CuSO4(s) in the CuSO4 solution? b dissolve some additional Zn(NO3)2(s) in the Zn(NO3)2 solution? c add H2O to the CuSO4 solution? d remove the salt bridge?
A potential of 0.142 V is recorded (under standard conditions) for a voltaic cell constructed using the following half reactions: Cathode: Pb2+(aq) + 2 e Pb(s) Anode: PbCl2(s) + 2 e Pb(s) + 2 Cl(aq) Net: Pb2+(aq) + 2 Cl(aq) PbCI2(s) (a) What is the standard reduction potential for the anode reaction? (b) Calculate the solubility product, Ksp, for PbCl2.
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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