Chemistry Please solve the questions as soon as possible. I'll upvote your work.Thank you! Ex 11. Write the scheme of a galvanic cell consisting of an electrode of the first kind and a redox electrode (optional of the above). Express the half-reactions occurring at each of the electrodes and the total reaction occurring in the element. Calculate the electrode potentials, the standard electromotive voltage of the element and AG 298 (t=25°C). Justify your answer! Zn/ZnCl(a=0.1M); = -0,76V = 0.22V Z AIO Ag/AgCl(TB),KCI (a=0.1M): PU/Fe (0.1M), Fe (0.05M); P=0.75V Li/LINO,(a-0.05M); -3.05V 4 14

Chemistry Please solve the questions as soon as possible. I'll upvote your work.Thank you! Ex 11. Write the scheme of a galvanic cell consisting of an electrode of the first kind and a redox electrode (optional of the above). Express the half-reactions occurring at each of the electrodes and the total reaction occurring in the element. Calculate the electrode potentials, the standard electromotive voltage of the element and AG 298 (t=25°C). Justify your answer! Zn/ZnCl(a=0.1M); = -0,76V = 0.22V Z AIO Ag/AgCl(TB),KCI (a=0.1M): PU/Fe (0.1M), Fe (0.05M); P=0.75V Li/LINO,(a-0.05M); -3.05V 4 14

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 14P

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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?
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
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).
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).
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?
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.