Two electrolytic cells containing silver nitrate solution and dilute sulphuric acid solution were connected in series. A steady current of 2.5 amp was passed through them till 1.078 g of silver was deposited. [Ag=107.8 g `mol^(-1)`,1 F=96,500 C]
(i) How much electricity was consumed ?
(ii) What was the weight of oxygen gas liberated ?

Explanation

To solve the problem step by step, we will address each part of the question separately.

### Part (i): How much electricity was consumed?

1. **Determine the number of moles of silver deposited**:
- The molar mass of silver (Ag) is given as 107.8 g/mol.
- The mass of silver deposited is 1.078 g.
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