Exactly 0.2 mole electrons are passed through two electrolytic cells in series containing `CuSO_(4)` and `ZnSO_(4)` respectively. How many grams of each metal will be deposited on the respective cathodes in the two cells ?

Explanation

To solve the problem, we need to determine how many grams of copper (Cu) and zinc (Zn) will be deposited when 0.2 moles of electrons are passed through the electrolytic cells containing CuSO₄ and ZnSO₄, respectively.

### Step-by-Step Solution:

**Step 1: Understand the Electrochemical Reactions**
- In the CuSO₄ cell, copper ions (Cu²⁺) are reduced to copper metal (Cu) at the cathode.
- In the ZnSO₄ cell, zinc metal (Zn) is oxidized to zinc ions (Zn²⁺) at the anode.

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