An electric current is passed through three cells connected in series containing `ZnSO_(4)`, acidulated water and `CuSO_(4)` respectively. What amount of Zn and `H_(2)` are liberated when 6.25 g of Cu is deposited? Eq. wt. of `Cu` and `Zn` are 31.70 and 32.6 respectively.

Explanation

To solve the problem, we need to determine the amounts of Zn and H₂ liberated when 6.25 g of Cu is deposited in the electrochemical cells. We will use the concept of equivalents in electrochemistry.

### Step-by-Step Solution:

1. **Identify the Equivalent Weights**:
- The equivalent weight of Copper (Cu) = 31.70 g/equiv
- The equivalent weight of Zinc (Zn) = 32.6 g/equiv
- The equivalent weight of Hydrogen (H₂) = 1 g/equiv
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