How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO₃(aq) using a current of 6.0 A

Question

Quizplus · Accepted Answer

We can use the equation:
moles of metal = (current x time)/(Faraday's constant x charge on ion)

The charge on Ag+ ion is +1, so the charge on Ag ion is 0 (since it is neutral).
The Faraday's constant is 96500 C/mol.

Substituting the values,
moles of metal = (6.0 A x 1.2 hours x 3600 s/h)/(96500 C/mol x 1)
moles of metal = 0.27 mol

Therefore, the answer is C) 0.27 mol.

How Many Moles of Silver Metal Are Produced in 1