A current of 4.60 A is passed through a Cr(NO3)2 solution for 1.10 hours. How much chromium is plated out of the solution?
each Cr ion needs two electrons.
Number of electrons: Current*time/chargeonElectron
4.6*1.1*60SECONDS/e
put the charge on an electron e in, and compute.
Then
massCr=molesCr*molmassCr
where molesCr=numberElectrons/2*1/avagnumber
To calculate the amount of chromium plated out of the solution, we need to use Faraday's Law of Electrolysis. According to Faraday's Law, the amount of a substance deposited or liberated during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
The formula for calculating the amount of substance plated out is as follows:
Amount of substance = (Current × Time) / (Number of electrons × Faraday's constant)
Now, let's break down the provided information:
Current = 4.60 A (amperes) (the rate of flow of electric charge)
Time = 1.10 hours (the duration of the current passing through the solution)
Number of electrons = The balanced chemical equation will provide this information.
Faraday's constant = A constant value representing the charge of one mole of electrons. Its value is 96,485 Coulombs/mol.
To calculate the amount of chromium plated out of the solution, we need to determine the number of electrons transferred during the electrochemical reaction. The balanced chemical equation for the electrolysis of Cr(NO3)2 solution can help us determine this.
Let's assume the balanced equation for the deposition of chromium during the electrolysis process is as follows:
2 Cr3+ + 6 e- -> 2 Cr
From the balanced equation, we can see that for every 6 electrons, 2 moles of Cr are plated out.
Now we can substitute the values into the formula:
Amount of substance = (Current × Time) / (Number of electrons × Faraday's constant)
Amount of substance = (4.60 A × 1.10 hours) / (6 × Faraday's constant)
Finally, we can calculate the amount of chromium plated out of the solution using the provided information.