worksheet3_ans-1 - Electrochemistry use of spontaneous...

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Electrochemistry – use of spontaneous chemical reactions to produce electricity but also using electricity to drive non-spontaneous reactions forward Galvanic cell – electrochemical cell in which a spontaneous chemical reaction generates an electric current Electrons are drawn into the cell through the cathode where reduction occurs and releases electrons at the anode Electrolytic Cell – have positive Gibb’s free energy with a negative E ° cell, non- spontaneous; external electrical power source is needed Anode – electrode where oxidations takes place Cathode – electrode where reduction takes place Cell potential – ability of a cell reaction to force electrons through a circuit (unit – Volt) 1 V x C = 1 J Δ G = -nFE F = Faraday’s constant = 96,500 C/mol e- Standard potential, E ° – measure of the electron-pulling power of a single electrode 12.6 Balance the following equations that take place in a basic solution. a) Cl 2 O 7 + H 2 O 2 b ClO 2 - + O 2 Net: Cl 2 O 7 + 4H 2 O 2 + 2OH - b 2ClO 2 - + 4O 2 + 5H 2 O b) MnO 4 - + S 2- b S + MnO 2 Net: 2MnO 4 - + 4H 2 O + 3S 2- b 3S
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This note was uploaded on 12/16/2010 for the course CHEM 6C CHEM 6C taught by Professor Pomeroy during the Spring '10 term at UCSD.

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worksheet3_ans-1 - Electrochemistry use of spontaneous...

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