12. Consider the electrochemical cell depicted below. Voltmeter NaC Ca(s) Al (s) Al(NO,), (aq) Cd(NO, (aq) a. Write an overall balanced chemical equation for the redox reaction taking place. b. What is oxidized what is reduced? C. CLEARLY label the following on the diagram of electrochemical cell abo i) the anode and the cathode ii) the direction electrons flow iii) the direction Na flows through the salt bridge iv) the direction Cl flows through the salt bridge

12. Consider the electrochemical cell depicted below. Voltmeter NaC Ca(s) Al (s) Al(NO,), (aq) Cd(NO, (aq) a. Write an overall balanced chemical equation for the redox reaction taking place. b. What is oxidized what is reduced? C. CLEARLY label the following on the diagram of electrochemical cell abo i) the anode and the cathode ii) the direction electrons flow iii) the direction Na flows through the salt bridge iv) the direction Cl flows through the salt bridge

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter13: Electrochemistry

Section: Chapter Questions

Problem 13.97PAE: As the voltaic cell shown here runs, the blue solution gradually gets lighter in color and the gray...

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A magnesium bar with a mass of 6.0 kg is attached to a buried iron pipe to serve as a sacrificial anode. An average current of 0.020 A flows between the bar and the pipe. (a) What reaction takes place at the surface of the magnesium bar? (b) What reaction takes place at the surface of the iron pipe? (C) In which direction do electrons flow between the two surfaces? (d) How many years would it take for the entire magnesium bar to be consumed?
As the voltaic cell shown here runs, the blue solution gradually gets lighter in color and the gray solution gets darker. (a) What species is oxidized and what is reduced? (b) Which electrode is the anode and which is the cathode? (C) Which metal electrode gains mass? (d) In which direction do electrons flow through the external circuit?
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Calculate the standard free energy change for the following reactions using the standard cell potentials for the half-reactions that are involved. (a) Fe(s)+Hg22+(aq)Fe2+(aq)+2Hg(l) (b Fe3+(aq)+Ag(s)+Cl-(aq)Fe2+(aq)+AgCl(s) (c) 2MnO4(aq)+5Zn(s)+16H3O+(aq)2Mn2+(aq)+5Zn2+(aq)+24H2O(l)
A mercury battery, used for hearing aids and electric watches, delivers a constant voltage (1.35 V) for long periods. The half-reactions are HgO(s)+H2O(l)+2eHg(l)+2OH(aq)Zn(s)+2OH(aq)Zn(OH)2(s)+2e Which half-reaction occurs at the anode and which occurs at the cathode? What is the overall cell reaction?
Why would a sacrificial anode made of lithium metal be a bad choice despite its ELi+/Li=2.07V, which appears to be able to protect all the other metals listed in the standard reduction potential table?
. In which direction do electrons flow in a galvanic cell, from anode to cathode or vice versa?
Which of the following statement(s) is/are true? a. Copper metal can be oxidized by Ag+ (at standard conditions). b. In a galvanic cell the oxidizing agent in the cell reaction is present at the anode. c. In a cell using the half reactions Al3+ + 3e Al and Mg2+ + 2e Mg, aluminum functions as the anode. d. In a concentration cell electrons always flow from the compartment with the lower ion concentration to the compartment with the higher ion concentration. e. In a galvanic cell the negative ions in the salt bridge flow in the same direction as the electrons.
Why is a salt bridge necessary in galvanic cells like the one in Figure 17.4?
Consider a salt bridge cell in which the anode is a manganese rod immersed in an aqueous solution of manganese(II) sulfate. The cathode is a chromium strip immersed in an aqueous solution of chromium(III) sulfate. Sketch a diagram of the cell, indicating the flow of the current throughout. Write the half-equations for the electrode reactions, the overall equation, and the abbreviated notation for the cell.
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