Calculate the number of coulombs required to deposit 5.4 g of Al when the electrode reaction is `Al^(3+)+3e^(-) to Al` (Given , atomic mass of Al =27 g `mol^(-1), F=96500 C mol^(-1)`)

Calculate the number of coulombs required to deposit 5.4 g of Al when

1.	Calculate the number of coulombs required to deposit 5.4 g of Al when the electrode reaction is `Al^(3+)+3e^(-) to Al` (Given , atomic mass of Al =27 g `mol^(-1), F=96500 C mol^(-1)`)
Answer» Correct Answer - `5.79xx10^(4) C` `Al^(3+)(aq)+underset(3xx96500C)(3e^(-)) to underset(27 g)(Al(s))` To deposit 27 g of Al(s), the amount of charge required `=3xx96500" C"` To deposit, 5.4 g of Al (s), the amount of charge required`=((3xx96500C))/((27 g))xx(5.4 g)=57900C=5.79xx10^(4)C`.

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Calculate the number of coulombs required to deposit 5.4 g of Al when the electrode reaction is `Al^(3+)+3e^(-) to Al` (Given , atomic mass of Al =27 g `mol^(-1), F=96500 C mol^(-1)`)

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