How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NICl2 for 60.0 minutes. Show all work.
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Coulombs = A x sec = 15A x 60 min x (60 sec/1 min) = about 54,000 but you need to go through and be more accurate.
96, coulombs will plate 1 equivalent of Ni. One equivalent is atomic mass/2 = about 58.7/2 = about 29g. Therefore, we can plate out
29 x (54,000/96,485) = about 16 g.
To calculate the number of grams of nickel metal plated out, you need to consider the amount of charge passing through the solution during the electrolysis process.
First, let's calculate the total charge passing through the solution using the formula:
Q = I * t
Where:
Q is the charge (in coulombs)
I is the current (in amperes)
t is the time (in seconds)
Since the current is given in amperes and the time is given in minutes, we need to convert the time to seconds:
60.0 minutes * 60 seconds/minute = 3600 seconds
Now, let's substitute the given values into the formula:
Q = 15.0 A * 3600 s = 54,000 C
Next, we need to calculate the number of moles of electrons involved in the electroplating reaction. In this case, we'll assume that the reduction of nickel(II) ions to nickel metal occurs with two electrons per ion:
2 moles of electrons = 1 mole of nickel(II) ions
Since the molar mass of nickel is 58.69 g/mol, we can use this information to find the amount of nickel metal plated out:
1 mole of nickel = 58.69 g
Now, let's calculate the number of moles of nickel metal:
moles of nickel = (1/2) * (54,000 C / 96,485 C/mol)
Dividing the charge by Faraday's constant (F), which is equal to 96,485 C/mol, gives us the number of moles of electrons involved.
moles of nickel = 0.559 mol
Finally, let's calculate the mass of nickel metal using the molar mass of nickel:
mass of nickel metal = moles of nickel * molar mass of nickel
mass of nickel metal = 0.559 mol * 58.69 g/mol
After performing the calculation, the mass of nickel metal plated out is approximately 32.77 grams.
To determine the number of grams of nickel metal plated out, we need to use Faraday's law of electrolysis. According to Faraday's law, the amount of substance (in grams) that is deposited or plated out during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
The formula for Faraday's law is:
mass = (Q * M) / (n * F)
Where:
- mass is the mass of the substance deposited or plated out (in grams),
- Q is the quantity of electricity passed (in coulombs),
- M is the molar mass of the substance (in grams per mole),
- n is the number of electrons transferred in the reaction, and
- F is Faraday's constant, which is approximately 96,500 coulombs per mole.
First, we need to find the quantity of electricity passed (Q). This can be calculated by multiplying the current (I) by the time (t):
Q = I * t
Given that the current is 15.0 A and the time is 60.0 minutes, we need to convert minutes to seconds (since current is given in amperes, which are measured per second):
Q = 15.0 A * 60.0 min * 60 s/min = 54,000 C
Now, we can calculate the molar mass of nickel metal (M). The molar mass of nickel is approximately 58.6934 grams per mole.
Next, we need to determine the number of electrons transferred in the oxidation-reduction reaction. For the reduction of nickel(II) ions to nickel metal, two electrons are transferred:
n = 2
Finally, we can substitute the values into the formula to calculate the mass of nickel metal:
mass = (Q * M) / (n * F)
mass = (54,000 C * 58.6934 g/mol) / (2 * 96,500 C/mol)
mass ≈ 31.87 g
Therefore, approximately 31.87 grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NICl2 for 60.0 minutes.