For each item, indicate if it is true for galvanic cells only, electrolytic cells only, both or neither (for a system not at equilibrium) - Reduction occurs at the anode A. galvanic cells only ✓ Reduction occurs at the cathode B. electrolytic cells only Electrons flow from the anode to the cathode c. both Electrons flow from the cathode to the anode D. neither ✓ Anions move towards the anode Anions move towards the cathode The cathode has a positive sign - The cathode has a negative sign A Moving to another question will save this response.

For each item, indicate if it is true for galvanic cells only, electrolytic cells only, both or neither (for a system not at equilibrium) - Reduction occurs at the anode A. galvanic cells only ✓ Reduction occurs at the cathode B. electrolytic cells only Electrons flow from the anode to the cathode c. both Electrons flow from the cathode to the anode D. neither ✓ Anions move towards the anode Anions move towards the cathode The cathode has a positive sign - The cathode has a negative sign A Moving to another question will save this response.

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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Identify each statement as true or false. Rewrite each false statement to make it true. (a) Oxidation always occurs at the anode of an electrochemical cell. (b) The anode of a discharging voltaic cell is the site ofreduction and is negative. (c) Standard-state conditions for electrochemical cells are aconcentration of 1.0 M for dissolved species and a pressure of 1 bar for gases. (d) The potential of a voltaic cell does not change withtemperature. (e) All product-favored oxidation-reduction reactions have astandard cell potential Ecell, with a negative sign.
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?
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NiCad batteries are rechargeable and are commonly used in cordless appliances. Although such batteries actuallyfunction under basic conditions, imagine a voltaic cellusing the setup in the diagram shown. (a) Write a balanced net ionic equation depicting the reaction occurring in the cell. (b) What is oxidized? What is reduced? What is the reducing agent and what is the oxidizing agent? (c) Which is the anode and which is the cathode? (d) Calculate E for the cell. (e) Indicate the direction of electron flow in the external wire. (f) If the salt bridge contains KNO3, toward which compartment will the NO3 ions migrate?
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