A current of 9.65 A is drawn from a Daniel cell for exactly one hour. Given molar masses of Cu and Zn a 63.5 g mol−1 and 65.4 g mol−1 respectively, the decreases in the mass of anode and increase in the mass of cathode will be respectively:
A
11.43g, 11.77g
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B
11.77g, 11.43g
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C
22.86g, 23.54g
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D
23.45g, 22.86g
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Solution
The correct option is B11.77g, 11.43g
The reaction occurring in Daniell cell is Zn+Cu2+→Zn2++Cu Zine is lost at anode and Cu is deposited at cathode amount of current with drawn is ((9.65A)(60×60S)/96500Cmol−1), which is 0.36 mol, Since two electrons are involved in the reduction and oxidation reaction, 0.18 ml of Zn is lost at anode and 0.18 mol of Cu is deposited at cathode. The masses are 11.77g and 11.43g for Zn and Cu respectively.