Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): Pt Cr 0.10 M MnO4 0.40 M Cr*+ 0.20 M Mn²+ 0.30 M Cr2O7²- 0.010 M H* 0.010 M H* The standard reduction potentials are as follows: MnO4¯ + 8H* + 5e Cr2072 + 14H* + 6e → Mn+ + 4H2O, ɛ° = 1.51 V 2Cr3+ + 7H2O, ɛ° = 1.33 V %3D 5. In the balanced cell reaction, what is the stoichiometric coefficient for H*? a. 5 b. 6 c. 30 d. 22 e. 2

Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): Pt Cr 0.10 M MnO4 0.40 M Cr+ 0.20 M Mn²+ 0.30 M Cr2O7²- 0.010 M H 0.010 M H* The standard reduction potentials are as follows: MnO4¯ + 8H* + 5e Cr2072 + 14H* + 6e → Mn+ + 4H2O, ɛ° = 1.51 V 2Cr3+ + 7H2O, ɛ° = 1.33 V %3D 5. In the balanced cell reaction, what is the stoichiometric coefficient for H*? a. 5 b. 6 c. 30 d. 22 e. 2

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

Section17.4: Voltaic Cells And Cell Potential

Problem 17.4PSP: Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the...

See similar textbooks

Similar questions

The standard potential for the reduction of AgSCN is 0.0895 V. AgSCN(s)+eAg(s)+SCN(aq) Find another electrode potential to use together with the above value and calculate Kspfor AgSCN.
Consider a galvanic cell based on the following half-reactions: a. What is the standard potential for this cell? b. A nonstandard cell is set up at 25C with [Mg2+] = 1.00 105 M. The cell potential is observed to be 4.01 V. Calculate [Au3+] in this cell.
The standard potential of the cell reaction Ag+(aq)+Eu2+(aq)Ag(s)+Eu3+(aq) is E = +1.23 V. Use the tabulated standard potential of the silver half-reaction to find the standard reduction potential for the europium half-reaction.
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.
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?
You want to set up a series of voltaic cells with specific cell potentials. A Zn2+(aq, 1.0 M)| Zn(s) half-cell is in one compartment. Identify several half-cells that you could use so that the cell potential will be close to (a) 1.1 V and (b) 0.50 V. Consider cells in which the zinc cell can be either the cathode or the anode.
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)?
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 the cell: Cr|Cr3+Co2+|Co E° is 0.46 V. The same cell was prepared in the laboratory at standard conditions. The voltage obtained was 0.40 V. A possible explanation for the difference is (a) the surface area of the chromium electrode was smaller than the cobalt electrode. (b) the mass of the chromium electrode was larger than the mass of the cobalt electrode. (c) the concentration of Cr(NO3)2 solution used was less than 1.0 M. (d) the concentration of Cr(NO3)2 solution used was less than 1.0 M. (e) the volume of Cr(NO3)2 solution used was larger than the volume of Cr(NO3)2 solution used.