The electrochemical equivalent of silver is 0.0012gC-1. If 36.0g of silver is to be deposited by electrolysis on a surface by passing a steady current for 5...

The electrochemical equivalent of silver is 0.0012gC-1. If 36.0g of silver is to be deposited by electrolysis on a surface by passing a steady current for 5.0mins, the current must be

Answer Details

The electrochemical equivalent of silver (Ag) is the amount of Ag deposited on a surface per unit charge passed through an electrolytic cell. It is given as 0.0012 gC-1. To find the current required to deposit 36.0g of Ag on a surface by electrolysis in 5.0 minutes, we can use the following formula: Current (I) = (mass of substance deposited)/(electrochemical equivalent × time) Substituting the given values, we get: I = (36.0 g)/(0.0012 gC-1 × 5.0 × 60 s) Simplifying this expression, we get: I = 100 A Therefore, the current required to deposit 36.0g of Ag on a surface by electrolysis in 5.0 minutes is 100 A.