Question

100. What mass (in g) of silver can be electroplated when 0.406 amps are used for 1.011 hours using a solution of silver nitrate?

Answer 1

Electrolysis equation is:
Ag1+   +   1e-    ------> Ag

1 mol of Ag requires 1 mol of electron
1 mol of electron = 96485 C
So,1 mol of Ag requires 96485 C

let us calculate the charge passed:
t = 1.011 hr = 1.011*3600 s = 3639 s

time, t = 3639s

Q = I*t
= 0.406A * 3639s
= 1477.434 C

mol of Ag plated = 1477.434/96485 = 0.01531 mol
Molar mass of Ag = 107.9 g/mol

mass of Ag = number of mol * molar mass
= 0.01531 * 107.9
= 1.65 g

Answer: 1.65 g

Please let me know if you have any doubts by commenting on this answer. I reply very fast. Also please mark the answer as helpful, If it helped