Stainless steel is known and used for its ability to resist corrosion. More corrosion resistant stainless steels such as those used in building construction contain molybdenum as well as chromium. Chromium metal can be electroplated from an aqueous solution of potassium dichromate. A current of 6.00 A and a voltage of 4.5 V are used in the electroplating. The reduction half-reaction is: Cr₂07¹ (aq) + 14H+ + 12e → 2Cr(s) +7H₂O a. How many grams of chromium can be plated if the current is run for 48 minutes? b. How long will it take to completely convert 215 mL of 1.25 M K2Cr2O7 to elemental chromium?

Stainless steel is known and used for its ability to resist corrosion. More corrosion resistant stainless steels such as those used in building construction contain molybdenum as well as chromium. Chromium metal can be electroplated from an aqueous solution of potassium dichromate. A current of 6.00 A and a voltage of 4.5 V are used in the electroplating. The reduction half-reaction is: Cr₂07¹ (aq) + 14H+ + 12e → 2Cr(s) +7H₂O a. How many grams of chromium can be plated if the current is run for 48 minutes? b. How long will it take to completely convert 215 mL of 1.25 M K2Cr2O7 to elemental chromium?

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 89QAP: An electrolysis experiment is performed to determine the value of the Faraday constant (number of...

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An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
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How long would it take to electroplate a metal surface with 0.500 g nickel metal from a solution of Ni2+ with a current of 4.00 A?
Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and 25 C. Zn | Zn(OH)2(s) | OH(aq) || Cu(OH)2(s) | Cu(s) a. Write a balanced equation for the reaction that occurs at the cathode. b. Write a balanced equation for the reaction that occurs at the anode. c. Write a balanced chemical equation for the overall reaction. d. Determine the potential (in volts) of the cell.
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The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.
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