Lecture_Notes_102609b

Lecture_Notes_102609b - 4 (aq) be carried out, at a current...

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Concentration Cell y A concentration cell is composed of two compartments each containing Br 2 (l) and Br - (aq) . Determine the cell potentials under each of the following conditions. Br 2 (l) + 2 e - 2 Br - (aq) ε o = 1.09 V y [Br - ] in each compartment is 1.0 M y [Br - ] = 0.5 M and 0.05 M in each compartment.
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Electrolysis y Electrolysis – the process of electrical energy being converted into chemical energy y Electrolytic Cell – uses electrical energy to produce chemical change y Ampere – (A) a measure of current
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Electrolysis
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Electrolysis y We can use electrolysis to determine the gold content of a sample. The sample was dissolved, and all of the gold is converted to Au 3+ (aq) , which is then reduced back to Au (s) on a weighed electrode. The reduction half-reaction is Au 3+ (aq) + 3 e - Æ Au (s) . What mass of gold will be deposited at the cathode in 1.00 hour by a current of 1.50 A?
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Electrolysis y For how many minutes must the electrolysis of a solution of CuSO
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Unformatted text preview: 4 (aq) be carried out, at a current of 2.25 A, to deposit 1.00 g of Cu (s) at the cathode? Without doing detailed calculations, determine which of the following solutions will yield the greatest number of moles of metal at a platinum cathode during it electrolysis by a 1.50 A electric current for 30.2 min: CuSO4 AgNO3 Au Cl 3 M o re i n fo rm a ti n s . .. 16% 4% 17% 63% 1. CuSO 4 2. AgNO 3 3. AuCl 3 4. More information is required Electrolysis 1. Determine the mass of the element of interest. 2. Find moles of element of interest. 3. Determine the number of electrons requires to create number of moles determined in step 2. 4. Determine coulombs of charge required. 5. Use amperage to determine amount of time. y If you are given time and need to determine mass, follow the steps in reverse....
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This note was uploaded on 01/06/2011 for the course CHEM 105BLG at USC.

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Lecture_Notes_102609b - 4 (aq) be carried out, at a current...

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