Questions 39-41 cover quantitative aspects of electrolysis and metal plating Question 39: How many minutes will it take to plate out 12.0 g Ni from an aqueous NiCl2 solution using a current of 35.0 amps? Express your answer to 3 significant figures. minutes Check Reuse <> Embed Question 40: To produce aluminum from its ore, one must reduce Al3+ to Al solid in an electrolysis cell. How much aluminum in grams could be produced if 20.0 amps of current is passed through the cell in 2.50 hours? Express your answer to 3 significant figures. Check g aluminum Reuse <> Embed Question 41: It requires 80.0 minutes to plate out 15.09 g of chromium from an aqueous chromium solution using a current of 35.0 amps. What was the charge of the chromium ions in the solution? charge = Check Reuse <> Embed H-P H-P H-P

Questions 39-41 cover quantitative aspects of electrolysis and metal plating Question 39: How many minutes will it take to plate out 12.0 g Ni from an aqueous NiCl2 solution using a current of 35.0 amps? Express your answer to 3 significant figures. minutes Check Reuse <> Embed Question 40: To produce aluminum from its ore, one must reduce Al3+ to Al solid in an electrolysis cell. How much aluminum in grams could be produced if 20.0 amps of current is passed through the cell in 2.50 hours? Express your answer to 3 significant figures. Check g aluminum Reuse <> Embed Question 41: It requires 80.0 minutes to plate out 15.09 g of chromium from an aqueous chromium solution using a current of 35.0 amps. What was the charge of the chromium ions in the solution? charge = Check Reuse <> Embed H-P H-P H-P

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions

Section: Chapter Questions

Problem 48PS: In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using...

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In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?
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?
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?
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 active (metal) electrode was found to lose mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode part of the anode or cathode? Explain.
The equation G = nF also can be applied to half-reactions. Use standard reduction potentials to estimate Gf for Fe2+ (aq) and Fe3+ (aq). Gf for e= 0.)
Consider the following electrochemical cell: a. If silver metal is a product of the reaction, is the cell a galvanic cell or electrolytic cell? Label the cathode and anode, and describe the direction of the electron flow. b. If copper metal is a product of the reaction, is the cell a galvanic cell or electrolytic cell? Label the cathode and anode, and describe the direction of the electron flow. c. If the above cell is a galvanic cell, determine the standard cell potential. d. If the above cell is an electrolytic cell, determine the minimum external potential that must be applied to cause the reaction to occur.
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
What is electrochemistry? What are redox reactions? Explain the difference between a galvanic and an electrolytic cell.
Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the following questions. Give reasons for your answers. (Use data from Table 17-1.) a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by SO42 (aq) in acid? d. Which species can be reduced by Al(s)?
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?
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).