What current strength in amperes will be required to liberate 10g of iodine from potassium iodine solution in one hour (1=127, Faraday constant=96500)

Answer 1

First, calculate the number of moles of iodine needed to liberate 10g:

Molar mass of iodine (I2) = 2(127) = 254 g/mol
Number of moles of iodine = 10g / 254 g/mol = 0.03937 mol

Next, calculate the total charge needed to liberate this amount of iodine:

Number of electrons needed = 2 (since I2 is diatomic)
Total charge needed = Number of electrons needed x Faraday constant
Total charge needed = 2 x 96500 C/mol = 193000 C

Finally, calculate the current needed to deliver this charge in one hour:

Current (in amperes) = Total charge / Time
Current = 193000 C / 3600 s = 53.61 A

Therefore, a current of approximately 53.61 amperes will be required to liberate 10g of iodine from potassium iodine solution in one hour.