Question

When 4.86 ampere of current is passed through an electrolyte for 60 min, 3.626 gm of divalent metal is deposited. The gram atomic weight of metal is

Answer 1

Answer:

hey friend the answer is 40

hope it helps you

Answer 2

Answer:

he gram atomic weight of the metal is 63.55 g/mol.

Explanation:

From the above question,

They have given :

4.86 ampere of current is passed through an electrolyte for 60 min, 3.626 gm of divalent metal is deposited.

We have to find the gram atomic weight of metal.

The volume of electrical energy handed via the electrolyte can be calculated as:

           Quantity of electrical energy = Current x Time

In this case, the cutting-edge is 4.86 A and the time is 60 minutes (or 3600 seconds):

      Quantity of electrical energy = 4.86 A x 3600 s

      Quantity of electrical energy = 17496 C

The quantity of metallic deposited can be calculated the usage of the formula:

Amount of steel deposited = (Quantity of electrical energy x Equivalent weight of metal) / 96500

where 96500 is the Faraday steady and represents the quantity of cost carried by way of one mole of electrons.

In this case, the steel is divalent, so its equal weight is half of of its atomic weight. Let's anticipate the atomic weight of the metallic is "A". Then, the equal weight would be "A/2".

Substituting the values, we get:

          3.626 g = (17496 C x (A/2)) / 96500

Simplifying the equation, we get:

             A = (2 x 3.626 g x 96500) / (17496 C)

             A = 63.55 g/mol

Therefore, the gram atomic weight of the metal is 63.55 g/mol.

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