During a electrolysis experiment one silver electrode gained 0.0373 g, while the

Question

During a electrolysis experiment one silver electrode gained 0.0373 g, while the other silver electrode in the cell loses 0.0351 g. During the 5710 seconds it takes for this process to occur, the average current in the cell is 6.04 milliamps. What is the estimated value of the Faraday using the values for: a.) the electrode that gains silver? b.) the electrode that loses silver? How do I set this type of problem up?

Explanation / Answer

m = (It / F)(M/z) .....where m=mass gained or lost ; I = current in the cell ; t = time of process to occur ; F = faraday constant ; M/z = equivalent weight ......a) 0.0373 = [(6.04*10^-3*5710 )/F][107.868 ] ....==>F = 99,737 C mol^-1 .....similarly for b) 0.0351 = [(6.04*10^-3*5710 )/F][107.868 ] ....==>F = 105,988 C mol^-1 .......

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