A current of 96.5 amperes is passed for 18 minutes between nickel electrodes in 500 ml solution of 0.2M nickel nitrate.the molarity of solution after electrolysis is
0.92
To determine the molarity of the solution after electrolysis, we need to calculate the moles of nickel nitrate that undergo electrochemical reaction.
First, let's calculate the charge passed during electrolysis using the formula:
charge (Coulombs) = current (Amperes) * time (seconds)
Since the current was given in amperes and the time was given in minutes, we need to convert the time to seconds:
time (seconds) = 18 minutes * 60 seconds/minute
time (seconds) = 1080 seconds
Now, we can calculate the charge passed:
charge (Coulombs) = 96.5 amperes * 1080 seconds
charge (Coulombs) = 104220 Coulombs
Next, we need to find the number of moles of electrons transferred during electrolysis. To do this, we can use Faraday's constant, which is 1 mole of electrons equal to 96485 Coulombs.
moles of electrons = charge (Coulombs) / Faraday's constant
moles of electrons = 104220 Coulombs / 96485 Coulombs/mol
moles of electrons = 1.08 moles
Since 1 mole of nickel nitrate reacts to produce 1 mole of nickel ions (Ni^2+), the molarity of the nickel nitrate solution will be equal to the moles of nickel ions divided by the volume of the solution (in liters).
First, let's convert the volume from milliliters to liters:
volume (liters) = 500 ml * (1 L / 1000 ml)
volume (liters) = 0.5 L
Now we can calculate the molarity (M) of the solution:
molarity (M) = moles of nickel ions / volume (liters)
molarity (M) = 1.08 moles / 0.5 L
molarity (M) = 2.16 M
Therefore, the molarity of the solution after electrolysis is 2.16 M.