A current of 5.41 A is pass through a Ni(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 7.30 g of nickel?

You may not be able to post for a few days but I think you can read responses. Here is how you do this problem.

You want 7.30g Ni.
96,485 coulombs will deposit 58.7g/2 or 29.35g Ni. so you will need
96,485 coulombs x (7.35/29.35) = approx 24,000 coulombs but that's an estimate and you should redo this calculation as well as all that follow.

Coulombs = amperes x seconds.
You know coulombs and amperes, solve for seconds and convert to hours.

To determine the time required to plate out 7.30 g of nickel, you need to use Faraday's law of electrolysis, which states:

Amount of substance deposited = (Electric current × Time × Atomic weight) / (Valency × Faraday's constant)

In this case, we are given the electric current (5.41 A) and the amount of nickel to be plated out (7.30 g). Let's solve for time:

1. Determine the atomic weight of nickel (Ni). The atomic weight of nickel is 58.69 g/mol.

2. Determine the valency of nickel in the Ni(NO3)2 solution. In this case, nickel has a valency of 2 since the compound is Ni(NO3)2.

3. Determine the Faraday's constant, which is 96,485 C/mol.

4. Rearrange the formula to solve for time:

Time = (Amount of substance deposited × Valency × Faraday's constant) / (Electric current × Atomic weight)

Plugging in the values:
Time = (7.30 g × 2 × 96,485 C/mol) / (5.41 A × 58.69 g/mol)

5. Calculate the time by solving the equation above:

Time = (2.0 × 7.30 g × 96,485 C/mol) / (5.41 A × 58.69 g/mol)

Time = 50,510.2 C / 315.1629 A

Time ≈ 160.33 s

Since the time is given in seconds, we need to convert it to hours:

Time = 160.33 s × (1 min / 60 s) × (1 hour / 60 min)

Time ≈ 0.0445 hours

So, the current would have to be applied for approximately 0.0445 hours to plate out 7.30 g of nickel.

To calculate the time required to plate out a given amount of nickel, we need two pieces of information - the amount of charge and the Faraday's constant.

The amount of charge (Q) is determined using the formula:
Q = I * t

where:
Q = amount of charge (in coulombs)
I = current (in amperes)
t = time (in seconds)

The Faraday's constant (F) relates the amount of charge to the amount of substance:
1 mole of electrons = 1 Faraday = F coulombs

Now, we can calculate the amount of charge required to plate out 7.30 g of nickel using the molar mass of nickel (58.6934 g/mol):
Q = (molar mass of nickel * mass of nickel) / (number of moles of electrons)

To find the number of moles of electrons, we need to know the balanced equation for the plating of nickel. Assuming it is:

Ni^2+ + 2e^- -> Ni (s)

From the equation, we can see that 2 moles of electrons are required to plate 1 mole of nickel.

Using these values, we can determine the amount of charge required. Then, dividing the charge by the current will give us the time required in seconds. Finally, we can convert the time to hours.

Let's calculate it step by step:

1. Calculate the number of moles of nickel:
moles of nickel = mass of nickel / molar mass of nickel

2. Calculate the number of moles of electrons:
moles of electrons = 2 * moles of nickel

3. Calculate the amount of charge required:
Q = moles of electrons * Faraday's constant (F)

4. Calculate the time required:
t = Q / I

5. Convert the time to hours:
time (hours) = t / 3600

Plugging in the values:

1. moles of nickel = 7.30 g / 58.6934 g/mol
2. moles of electrons = 2 * moles of nickel
3. Q = moles of electrons * Faraday's constant (F)
4. t = Q / I
5. time (hours) = t / 3600

Now, let's calculate it step by step.

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