How many moles of electrons are required to produce 23.8 g Cu from a CuSO4 solution?

96,485 coulombs are required to produce 1/2 mole Cu(63.546g/2); therefore, x coulombs are required to produce 23.8 g Cu. There are 6.022 x 10^23 electrons in 96,485 coulombs.

To determine how many moles of electrons are required to produce 23.8 g of Cu from a CuSO4 solution, we need to use the concept of stoichiometry and Faraday's law of electrolysis.

Here's the step-by-step process to find the answer:

1. Find the molar mass of Cu:
The molar mass of Cu is 63.55 g/mol. This value can be found in the periodic table.

2. Convert grams of Cu to moles of Cu:
Use the following formula:
Moles = Mass (g) / Molar Mass (g/mol)
Moles = 23.8 g / 63.55 g/mol
Moles = 0.375 mol

3. Determine the stoichiometry of the reaction:
The balanced equation for the reaction is:
2e- + Cu2+ → Cu
This means that 2 moles of electrons are required to produce 1 mole of Cu.

4. Calculate the moles of electrons required:
Use the stoichiometry ratio to convert moles of copper to moles of electrons:
Moles of electrons = Moles of Cu × (2 moles of electrons / 1 mole of Cu)
Moles of electrons = 0.375 mol × 2
Moles of electrons = 0.75 mol

Therefore, 0.75 moles of electrons are required to produce 23.8 g of Cu from a CuSO4 solution.