0.222g of a divalents metal is deposited when a current of 0.45a is passed through a solution of it salts for 25mins calculate the relative atomic mass of the metal (1faraday =96500c)
an ampere is a coulomb per second
0.45 coul/s * 60 s/min * 25 min = ? coulombs
6.2E18 electrons per coulomb
... divide by Avogadro's number to find moles of electrons
it takes two electrons to deposit one atom of the metal (DIvalent)
find the moles of metal
divide sample mass by moles of metal to find atomic mass
To calculate the relative atomic mass of the metal, we need to use the concept of Faraday's law of electrolysis.
Step 1: Convert the given current from amperes (A) to coulombs per second (C/s):
I = 0.45 A
Step 2: Calculate the total charge passed through the solution using the formula:
Q = I * t
where Q is the charge passed (in coulombs) and t is the time (in seconds).
Given:
t = 25 minutes = 25 * 60 seconds
Q = 0.45 A * 25 * 60 s
Step 3: Calculate the moles of electrons involved in the reaction using Faraday's law of electrolysis:
1 mole of electrons = 1 Faraday = 96500 C
Moles of electrons = Q / 96500
Step 4: Convert the mass of the metal deposited to moles using the concept of molar mass.
The atomic mass unit (AMU) is defined as the mass equal to 1/12th the mass of carbon-12. This means that 1 AMU is equal to 1 gram per mole (g/mol).
Given: Mass of metal = 0.222 g
Measure the valency of the metal
Since the metal is divalent, the moles of electrons will be equal to half of the moles of the metal.
Moles of metal = Moles of electrons / 2
Step 5: Calculate the relative atomic mass (RAM) using the formula:
RAM = Mass of metal / Moles of metal
Therefore, by following these steps, you can calculate the relative atomic mass of the metal.