A current of 3.40 A is passed through a Ni(NO3)2 solution for 1.80 hours. How much nickel is plated out of the solution?
Made a mistake that Dr. Bob222 caught in an earlier post. See your earlier post for corrections.
Current=charge/time (s)
Where
current=3.40A
Convert hr to seconds (s):
1.80hrs*(60 min/1 hr)*(1 min/60s)= time in s
Solve for charge:
seconds*current=charge (C)
1 mole of e^-s=9.65 x 10^4 C
Solve for moles:
C*(1 mole/9.65 x 10^4 C)=moles of e^-s
The half reaction is the following:
Ni2+ + 2e ---> Ni
So, 2 moles of e^- is needed for 1 mole of Ni:
Solve for moles of Ni:
moles of e^-s*(1 mole of Ni/2 mole of e^-)= moles of Ni
Solve for mass:
moles of Ni*( 58.69 g/mole)= mass of Ni
I am doing something wrong I keep getting the wrong answer
Instead of us guessing, why don't you show your work so we can find the error.
To find out the amount of nickel that is plated out of the solution, we need to use Faraday's Law of Electrolysis. Faraday's Law states that the amount of substance deposited or liberated at an electrode is directly proportional to the quantity of electricity passed through it.
The equation to calculate the amount of substance deposited is:
Mass (in grams) = (current (in amperes) × time (in seconds) × molar mass of the substance) / (number of moles of electrons × Faraday's constant)
In this case, we're plating nickel from the Ni(NO3)2 solution, so we need to know the molar mass of nickel. The molar mass of nickel (Ni) is approximately 58.69 g/mol.
Now let's calculate the number of moles of electrons involved in the reaction. We need to calculate the oxidation state of nickel in the Ni(NO3)2 solution. In this case, nickel is being reduced, and its oxidation state is +2. When nickel is reduced, it gains two electrons.
Using Faraday's constant, which is approximately 96,485 C/mol, we can calculate the mass of nickel plated out of the solution.
First, we need to convert the time from hours to seconds:
Time = 1.80 hours × 3600 seconds/hour = 6480 seconds
Now we can plug the values into the equation:
Mass (in grams) = (3.40 A × 6480 s × 58.69 g/mol) / (2 × 96,485 C/mol)
By calculating this expression, we can find the amount of nickel that is plated out of the solution.