Problem: A current of 3.07 A is passed through a Pb(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 7.10 g of lead?

FREE Expert Solution

We have to calculate the time required to deposit 7.10 g of lead metal from a solution containing Pb(NO3)2.


  • The time required to deposit a substance on an electrode can be determined through the use of Faraday’s constant.
  • Faraday’s constant is defined as 9.648x104 C charge per mol of e-.
  • NO3- is a polyatomic ion with a charge of -1.
  • Pb(NO3)2 has 2 NO3- ions therefore the negative charge is -2.
  • To balance this negative charge, a charge of +2 on Pb is required.


Pb2+ has a +2 charge, so it requires 2 electrons to discharge completely and deposit as a metal.


Pb2+(aq) + 2e- → Pb(s)


View Complete Written Solution
Problem Details

A current of 3.07 A is passed through a Pb(NO3)solution. How long (in hours) would this current have to be applied to plate out 7.10 g of lead?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Faraday's Constant concept. You can view video lessons to learn Faraday's Constant. Or if you need more Faraday's Constant practice, you can also practice Faraday's Constant practice problems.