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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 0.783g. calculate the equivalent mass of the metal. |
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Answer» I = 0.15 amperes t = 150 mins = t = 150 x 60sec = t = 9000sec Q = It = Q = 0.15 x 9000 coulombs = Q = 1350 coulombs Hence, 135 coulombs of electricity deposit is equal to 0.783g of metal. 96500 coulombs of electricity \(\frac{0.783\times96500}{1350}\) = 55.97 gm of metal Hence equivalent mass of the metal is 55.97 I = 0.15 amperes t = 150 mins = t = 150 x 60sec = t = 9000sec Q = It = Q = 0.15 x 9000 coulombs = Q = 1350 coulombs Hence, 135 coulombs of electricity deposit is equal to 0.783g of metal. 96500 coulombs of electricity 0.783×9650013500.783×965001350 = 55.97 gm of metal Hence equivalent mass of the metal is 55.97 |
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