A current of 96.5 A is passed for 18 min between nickel electrodes in 500 mL solution of 2M Ni(NO3)2. The molarity of solution after electrolysis would be
To determine the molarity of the solution after electrolysis, we need to consider the changes that occur during the electrolysis process.
First, let's calculate the amount of charge (Q) that passes through the electrolyte using the formula:
Q = I * t
where Q represents the charge in Coulombs (C), I is the current in Amperes (A), and t is the time in seconds (s).
Given:
I = 96.5 A
t = 18 min = 18 * 60 = 1080 s
So, Q = 96.5 A * 1080 s = 104220 C
Next, we need to determine the number of moles of electrons (n) that were transferred during the electrolysis. This can be done using Faraday's law:
n = Q / F
where F represents Faraday's constant, which is equal to 96500 C/mol.
n = 104220 C / 96500 C/mol ≈ 1.08 mol
During the electrolysis of Ni(NO3)2, 2 moles of electrons are required to reduce 1 mole of Ni2+ ions. Therefore, the number of moles of Ni2+ ions that were reduced is half the number of moles of electrons:
moles of Ni2+ ions = n / 2
moles of Ni2+ ions = 1.08 mol / 2 = 0.54 mol
Finally, we can calculate the new molarity of the solution by considering the volume of the solution and the number of moles of the solute:
Molarity = moles of solute / volume of solution
Given:
Volume of solution = 500 mL = 500 / 1000 = 0.5 L
Molarity = 0.54 mol / 0.5 L = 1.08 M
Therefore, the molarity of the solution after electrolysis would be approximately 1.08 M.