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A solution of a salt of metal was electrolysed for 150 minutes with a current of 0.15 amperes. The mass of the metal deposited at the cathode is 0.783 g. Calculate the equivalent mass of the metal. |
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Answer» Solution :Given `I = 0.15` amperes `t = 150` mins `implies t = 150 XX 60 "sec" implies t = 9000` sec `Q = I t implies Q = 0.15 xx 9000` coulombs `implies Q = 1350` coulombs Hence, `135` coulombs of electricity DEPOSITE is EQUAL to `0.783 g` of metal. `:. 96500` coulombs of electricity , `(0.783 xx 96500)/(1350) = 55.97` gm of metal Hence equivalent mass of the metal is `55.97`. |
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