ws13302 - CH 302 Worksheet 13 More Advanced...

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CH 302 Worksheet 13 More Advanced Electrochemistry calculations 1. (a) Calculate the mass of copper metal produced at the cathode during the passage of 2.50 amps of current through a solution of copper (II) sulfate for 50.0 minutes. (b) What volume of oxygen gas (measured at STP) is produced by the oxidation of water at the anode in the electrolysis of copper(II) sulfate in part (a)? 2. What is the E ° for the following electrochemical cell where Zn is the cathode? Zn | Zn 2+ (1.0 M ) || Fe 2+ (1.0 M ) | Fe E ° (Zn) = -0.76 E ° (Fe) = -0.44 3. For the electrolysis of molten sodium bromide, write the two half-reactions and show write which electrode at which each occurs (cathode or anode). 4. Calculate the potential, E , for the Fe 3+ / Fe 2+ electrode when the concentration of Fe 2+ is exactly five times that of Fe 3+ . Fe 3+ + e - Fe 2+ E ° = +0.771 V 5. At standard conditions, will chromium (III) ions, Cr 3+ , oxidize metallic copper to copper (II) ions, Cu 2+ , or will Cu 2+ oxidize metallic chromium to Cr
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This note was uploaded on 10/07/2011 for the course CHEMISTRY 51635 taught by Professor Laude during the Spring '10 term at University of Texas.

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ws13302 - CH 302 Worksheet 13 More Advanced...

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