Lesson_23_-_Example_solution_-2009

Lesson_23_-_Example_solution_-2009 - Lesson 23 Example 23-1...

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Lesson 23 Example 23-1 A galvanic cell consists of a cadmium cathode immersed in a CdSO 4 solution and a zinc anode immersed in a ZnSO 4 solution. A salt bridge connects the two half-cells. (a) Write a balanced equation for the cell reaction. (b) A current of 1.45 A is observed to flow for a period of 2.6 hours. How much charge has passed through the circuit during this time? How many moles of electrons is this charge equivalent to? (c) Calculate the change in the mass of the zinc electrode. (d) Calculate the change in the mass of the cadmium electrode. ____________________________________________________________________________________________ Solution: (a) Cathode: Cd 2+ ( aq ) + 2 e - Cd( s ) (reduction) Anode: Zn ( s ) Zn 2+ ( aq ) + 2 e - (oxidation) Cell reaction: Zn ( s ) + Cd 2+ ( aq ) Zn 2+ ( aq ) + Cd( s ) 1
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(b) ( 29 C 13572 h s 3600 h 6 . 2 s C 45 . 1 It Q = = = mol 141 . 0 mol
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Lesson_23_-_Example_solution_-2009 - Lesson 23 Example 23-1...

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