For Part a), we're being asked to calculate how many coulombs of charge is needed to produce 61.2 mol of solid zinc.
We're given the following reaction: Zn2+(aq) + 2e− → Zn(s)
• Zn(s) must be formed from Zn2+(aq)
• Zn2+ needs to gain 2 e- in order to become Zn(s)
We can now calculate the charge needed.
Step 1: Calculate the number of moles e- produced from the reaction (using mole-to-mole comparison)
Step 2: Calculate the charge needed (using Faraday’s constant)
Galvanized nails are iron nails that have been plated with zinc to prevent rusting. The relevant reaction is
Zn2+(aq) + 2e− → Zn(s)
For a large batch of nails, a manufacturer needs to plate a total zinc mass of 4.00 kg on the surface to get adequate coverage.
a. How many coulombs of charge are needed to produce 61.2 mol of solid zinc?
b. Identify the anode and cathode when plating an iron nail with zinc.
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 Electroplating concept. If you need more Electroplating practice, you can also practice Electroplating practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Korolev's class at UF.