0.222g of a divalent metal is deposited when a current of 0.45A is pass through a solution of it's salt for 25 minutes calculate the relative atomic mass of the metal (1 Faraday=96500c)
To calculate the relative atomic mass of the metal, we need to use Faraday's law of electrolysis.
According to Faraday's law, the amount of a substance deposited during electrolysis is directly proportional to the amount of charge passed through the solution. The formula for Faraday's law is:
Amount of substance (in mol) = (Current (in A) × Time (in s)) / (n × Faraday's constant)
In this case, we are given the current (0.45 A), time (25 minutes = 1500 s), and the mass of the metal deposited (0.222 g). We need to determine the value of n (the number of electrons transferred) for the metal.
Since the metal is divalent, it means that 2 moles of electrons are transferred per mole of metal deposited. Therefore, n = 2.
Now, we can rearrange the formula to solve for the relative atomic mass (RAM) of the metal:
RAM = (Mass of metal deposited / Amount of substance) × Molar mass
First, let's calculate the amount of substance:
Amount of substance = (0.45 A × 1500 s) / (2 × 96500 C/mol)
= 0.00439 mol
Next, we can use the molar mass of the metal to calculate the RAM. The molar mass can be determined using the mass of the metal deposited and the amount of substance:
Molar mass = Mass of metal deposited / Amount of substance
= 0.222 g / 0.00439 mol
= 50.570 g/mol
Therefore, the relative atomic mass of the metal is approximately 50.570.