How many minutes are needed to plate out 29.00g Mg from molten MgCl2, using 2.70A of current?

It takes 96,485 coulombs to plate out 1 equivalent weight of Mg which is 24.3/2 = 12.15g Mg. You want 29 g so it will take

96,485 x 29/12.15 = ? coulombs
amperes x seconds = coulombs.
You know amperes and coulombs, solve for seconds and convert to minutes.

17381

To find the number of minutes needed to plate out 29.00g of Mg using 2.70A of current, we need to use Faraday's Law of Electrolysis. The formula for Faraday's Law is:

moles of substance plated = (current * time) / (n * F)

where:
- moles of substance plated is the amount of substance being plated (in this case, Mg),
- current is the electric current used (2.70A),
- time is the time in seconds,
- n is the number of electrons transferred in the reaction (it is equal to the number of moles of electrons required),
- F is Faraday's constant (96,485 C/mol).

First, we need to determine the number of moles of Mg. We can calculate this using the molar mass of Mg, which is 24.31 g/mol.

moles of Mg = mass / molar mass
moles of Mg = 29.00g / 24.31 g/mol = 1.19 mol

Since the balanced chemical equation for the electrolysis of MgCl2 is:

2MgCl2(l) → 2Mg(l) + Cl2(g)

we can see that 2 moles of electrons are required for every mole of Mg plated.

Now we can substitute the values into Faraday's Law and solve for time (in seconds):

1.19 mol = (2.70A * time) / (2 mol * 96,485 C/mol)

Rearranging the formula, we get:

time = (1.19 mol * 2 mol * 96,485 C/mol) / 2.70A

Calculating this, we find:

time ≈ 517,150 seconds

Finally, we can convert seconds to minutes by dividing by 60:

time in minutes ≈ 517,150 seconds / 60 ≈ 8619 minutes

Therefore, it would take approximately 8619 minutes to plate out 29.00g of Mg from molten MgCl2 using 2.70A of current.

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