mass of the potassium formed by the passage of 5.92 amps for 1.94 hours through an electrolytic cell that contains a molten potassium salt is 16.41g
Total amount of current in amps = 5.92 Columbus/ sec(I)
total time period = 1.94 h = 1.94 X 3600 sec = 6984 sec(t)
initially electric charge Q is calculated Q =I X t =41,345.28 Columbus
now molar mass of K is 39.09g/mol and faradays constant = 96485 so by the formula , n=Q/F = 41,345.28/96485 =0.4285mol now, m = nM where n is number of mol and M is molar mass of K so 0.42 X 39.09=16.41g
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