Answer to Question #113504 in General Chemistry for Beverlie

Question

Suppose the current flowing from a battery is used to electroplate an object with silver. Calculate the mass of silver that would be deposited by a battery that delivers 1.25 A·hr of charge.

Answer 1

Solution.

$q=1.25A\sdot hr = 4500A\sdot s =4500Kl;$

By Faraday's law we find the mass of silver: $m=k\sdot q;$

The electrochemical equivalent of silver is: $k=1.118\sdot 10^{-6}kg/Kl;$

$m=1.118\sdot10^{-6}kg/Kl\sdot4500Kl =5.031\sdot10^{-6}kg =0.005g;$

Answer: $m=0.005g.$