homework11 - 2+ and Zn 2+ are 1.5M and 0.1M, respectively....

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Physical Chemistry I, Homework 11 7.1) For each of the redox reactions occurring in acidic solution: i) PbO 2 (s) + I - (aq) à Pb 2+ (aq)+I 2 (s) ii) SO 3 2- (aq)+MnO 4 - (aq) à SO 4 2- (aq)+Mn 2+ (aq) Do the following: a) Balance each of the redox reactions, b) sketch the corresponding voltaic cell, label the anode and cathode and indicate the half-reactions occurring at each electrode and the species present in each solution, indicate the direction of electron flow c) Write down the voltaic cell notation and calculate the E o d) Calculate the % r G o and equilibrium constant K at 25 o C. 7.2) A voltaic cell consists of a Zn 2+ /Zn and Ni 2+ /Ni half-cell at 25 o C. The initial concentrations of Ni
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Unformatted text preview: 2+ and Zn 2+ are 1.5M and 0.1M, respectively. a) what is the initial cell potential b) what is the cell potential when the concentration of Ni 2+ has fallen to 0.5M c) what are the concentration of Ni 2+ and Zn 2+ when the cell potential falls to 0.45V 7.3) The equlibrium constant of CuI is 1.1x10-12 , find the E o for the following cell Cu(s)|CuI(s)|I-(aq)(1M)||Cu + (aq)(1M)|Cu(s) 9 th edition: Exercises: 6.20,6.24 Problem 6.20 8 th edition Exercises 7.14, 7.18 Problem 7.20 Optional questions: 9 th edition : Exercises 6.19, 6.21,6.22 8 th edition: Exercises 7.13, 7.15, 7.16...
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This note was uploaded on 12/12/2011 for the course CHE 301 taught by Professor Raineri,f during the Fall '08 term at SUNY Stony Brook.

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homework11 - 2+ and Zn 2+ are 1.5M and 0.1M, respectively....

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