Question

A current is passed through three electrolytic cells connected in series containing solutions of silver trioxonitrate (v), copper (II)tetraoxosulphate (VI) and brine respectively. If 12.7g of copper are deposited in the second electrolytic cell, calculate :

A: the mass of silver deposited in the first cell
B:the volume of chlorine liberated in the third cell at 17°c and 800mmhg pressure.
(Ag=108,cu=63.5,1F=96500c,GMV of gas at S.T.P=22.4dm^3)?

Answer 1

To calculate the mass of silver deposited in the first cell, divide the total charge passed by the charge per mole of electrons, then use Faraday's law of electrolysis to determine the number of moles of silver deposited.

Step-by-step explanation:

To calculate the mass of silver deposited in the first cell, we need to first determine the number of moles of electrons that passed through the second cell.

Using the given charge of 96500 C/mole, we can calculate the number of moles of electrons by dividing the total charge passed (given as 12.7g * (1/63.5g/mole)) by the charge per mole of electrons.

Once we have the number of moles of electrons, we can use Faraday's law of electrolysis to determine the number of moles of silver deposited in the first cell.

Answer 2

Answer: check out the image

Explanation: check out the image