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?
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 Ni(NO3)2
Solve for mass:
moles of Ni(NO3)2*(182.703 g/mole)= mass of Ni(NO3)2
Note that there are two mols of electrons and you must take that into account. A minor problem is that you will not plate out Ni(NO3)2 but Ni metal.
Dr. Bob222 caught that for me. Look for **** 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
Dr. Bob222 is correct: the question states Ni not Ni(NO3)2.
To determine the amount of nickel plated out of the solution, we can use Faraday's Law of Electrolysis. Faraday's Law states that the amount of substance deposited (in this case, nickel) is directly proportional to the quantity of electricity passed through the solution.
The formula is given as:
Amount of substance deposited = (Current * Time) / (Faraday's constant * Charge of the substance)
Now, let's gather the given information:
Current (I) = 3.40 A
Time (t) = 1.80 hours
To proceed further, we need to determine the Faraday's constant and the charge of nickel.
According to Faraday's constant, 1 mole of electrons carries a charge of 96,485 C.
To find out the charge of nickel (Ni), we need to determine its oxidation state.
Nickel commonly has an oxidation state of +2. So, it requires 2 moles of electrons to plate 1 mole of nickel.
The molar mass of nickel (Ni) is 58.69 g/mol. Hence, 1 mole of nickel weighs 58.69 grams.
Using the above information, we can calculate the charge of nickel:
Charge of nickel = (2 moles of electrons * 96,485 C) / (1 mole of nickel)
Now, let's calculate the amount of nickel plated:
Amount of nickel plated = (Current * Time) / (Faraday's constant * Charge of nickel)
Substituting the given values, we can solve for the amount of nickel plated out of the solution.