What change in coulombs, is required to deposit 0.301 g Cu(s) from a solution of Cu^2+(aq)

Let's think it through step by step.

First convert 0.301g to moles of copper.
0.301 g /63.5 g/mole = 4.74*10^-3 moles.
Multiply that by 2 x (Avogadro's number) for the number of electrons.
Multiply what you get by the number of Coulombs per electron (1.602*10^-19).

I get 914 C

To determine the change in coulombs required to deposit 0.301 g of Cu(s) from a solution of Cu^2+(aq), we need to use Faraday's laws of electrolysis.

1. Determine the molar mass of copper (Cu).

The molar mass of Cu is 63.55 g/mol.

2. Use the molar mass to calculate the number of moles of Cu.

Number of moles = mass / molar mass = 0.301 g / 63.55 g/mol = 0.00473 mol

3. According to Faraday's laws of electrolysis, 1 mol of electrons is required to deposit 1 mol of Cu.

Therefore, the number of moles of electrons required is also 0.00473 mol.

4. Convert the number of moles of electrons to the number of coulombs using Faraday's constant.

According to Faraday's constant, 1 mole of electrons is equal to 96,485 coulombs.

Number of coulombs = number of moles of electrons × Faraday's constant
= 0.00473 mol × 96,485 coulombs/mol
≈ 454.94 coulombs

Therefore, approximately 454.94 coulombs of charge is required to deposit 0.301 g of Cu(s) from a solution of Cu^2+(aq).

To determine the change in coulombs required to deposit a certain amount of copper from a copper(II) solution, we need to use Faraday's law of electrolysis. The equation for Faraday's law is:

m = (Q * M) / (z * F)

Where:
- m is the mass of the substance being deposited or liberated (in this case, Cu)
- Q is the quantity of electricity passing through the solution (in coulombs)
- M is the molar mass of the substance (in g/mol)
- z is the number of moles of electrons involved in the reaction (in this case, 2 electrons for one mole of Cu^2+)
- F is the Faraday constant (approximately 96,485 C/mol)

Given that we want to deposit 0.301 g of Cu(s), the mass (m) in the equation will be 0.301 g. The molar mass of Cu is approximately 63.546 g/mol, so M will be 63.546 g/mol. Since Cu^2+ gains 2 electrons to form a solid copper, z will be 2. Finally, the Faraday constant (F) is approximately 96,485 C/mol.

Now, we can rearrange the equation to solve for Q:

Q = (m * z * F) / M

Plugging in the given values:

Q = (0.301 g * 2 * 96,485 C/mol) / 63.546 g/mol

Simplifying the expression:

Q = 0.301 g * 2 * 96,485 C/mol / 63.546 g/mol
Q = 0.301 * 2 * 96,485 / 63.546 C
Q ≈ 913.19 C

Therefore, approximately 913.19 coulombs of electric charge are required to deposit 0.301 g of Cu(s) from a solution of Cu^2+(aq).