0.222g of a divalent metal is deposited when a current of 0.45A is passed through a solution of its salt for 15min. Calculate the relative atomic mass of the metal. (1F =96500C)

Answer 1

First, let's calculate the charge that passed through the solution:

Charge = Current x Time
Charge = 0.45A x 15min
Charge = 6.75C

Next, we need to convert the charge to moles using Faraday's constant:

Moles = Charge / Faraday's constant
Moles = 6.75C / 96500C/mol
Moles = 0.00007mol

Since the metal is divalent, the number of moles of the metal is half of the number of moles of the charge, so:

Moles of metal = Moles / 2
Moles of metal = 0.00007mol / 2
Moles of metal = 0.000035mol

Next, we can calculate the mass of the metal:

Mass = Moles x Relative atomic mass
0.222g = 0.000035mol x Relative atomic mass

Rearranging the equation to solve for the relative atomic mass:

Relative atomic mass = 0.222g / 0.000035mol
Relative atomic mass = 6342.857

Therefore, the relative atomic mass of the metal is 6342.857.