0.222g of a divalent motal is deposited when g current of 0.45A is passed through a solution of its salt for 25 minutes. Calculate the relative atomic mas of the metal. ( 1 faraday = 96500c) .
First, we need to calculate the number of moles of the metal that are deposited using the formula:
moles = mass / molar mass
Given that the mass deposited is 0.222g and the current is 0.45A for 25 minutes, we can calculate the charge passed using the formula:
charge = current * time
charge = 0.45A * 25 minutes * 60 seconds/minute = 675 coulombs
Since 1 Faraday is equal to 96500 coulombs, we can convert the charge passed to Faradays:
charge in Faradays = charge / 96500 = 675 / 96500 = 0.006993 Faradays
Since each mole of a divalent metal requires 2 Faradays to be deposited, we can calculate the moles using the formula:
moles = charge in Faradays / 2 = 0.006993 / 2 = 0.003497 moles
Next, we need to calculate the relative atomic mass of the metal using the formula:
relative atomic mass = mass / moles
Given that the mass deposited is 0.222g and the moles are 0.003497, we can calculate the relative atomic mass:
relative atomic mass = 0.222g / 0.003497 = 63.5
Therefore, the relative atomic mass of the metal is 63.5.