A: One faraday electricity deposite 1 mole of Na & 2 mole of Cu in NaCl & `CuSO_(4)` solution respectively.
R: One faraday electricity always deposite 1 mole of any substance.

Answer

To solve the question, we will analyze both the assertion (A) and the reason (R) provided in the statement.

### Step 1: Understanding the Assertion (A)
The assertion states that "One faraday electricity deposits 1 mole of Na and 2 moles of Cu in NaCl and CuSO4 solution respectively."

- **For Sodium (Na)**: Sodium has a valency of +1, meaning that 1 mole of Na requires 1 Faraday of electricity to deposit.
- **For Copper (Cu)**: Copper (in CuSO4) has a valency of +2, meaning that 1 mole of Cu requires 2 Faradays of electricity to deposit. Therefore, 1 Faraday would deposit 0.5 moles of Cu.

### Step 2: Analyzing the Assertion
From the analysis:
- 1 Faraday deposits 1 mole of Na (correct).
- 1 Faraday deposits 0.5 moles of Cu (incorrect).

Thus, the assertion is incorrect because it states that 1 Faraday deposits 2 moles of Cu, which is not true.

### Step 3: Understanding the Reason (R)
The reason states that "One faraday electricity always deposits 1 mole of any substance."

This statement is also incorrect because the amount of substance deposited depends on the valency of the ions involved in the electrochemical reaction. Different substances require different amounts of Faraday to deposit 1 mole.

### Step 4: Conclusion
Both the assertion and the reason are incorrect. Therefore, the correct answer to the question is that both A and R are false.

### Final Answer
Both the assertion (A) and the reason (R) are false.

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