The amount of copper deposited by one Faraday current will be maximum in an acidic solution of one litre of-

Options

A. `1M Cu_(2)Cl_(2)`
B. `2M Cu(NO_(3)_(2))`
C. `5 M CuSO_(4)`
D. `5M Cu_(2)(PO_(4))_(2)`

Explanation

To determine the amount of copper deposited by one Faraday current in various acidic solutions, we need to consider the following steps:

### Step 1: Understand Faraday's Law of Electrolysis
Faraday's law states that the amount of substance deposited or liberated during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte. The relationship can be expressed as:
\[ m = \frac{Q}{F} \times \frac{M}{n} \]
where:
- \( m \) = mass of the substance deposited (in grams)
- \( Q \) = total electric charge (in coulombs)
- \( F \) = Faraday's constant (approximately 96500 C/mol)
- \( M \) = molar mass of the substance (in g/mol)
- \( n \) = number of electrons transferred per ion of the substance

### Step 2: Identify the Copper Compounds
We have the following copper compounds to consider:
1. Cu₂Cl₂
2. Cu₂O₃
3. Cu₄O₄
4. Cu₂P₄

### Step 3: Determine the Oxidation States
- In Cu₂Cl₂, copper is in the +1 oxidation state.
- In Cu₂O₃, copper is in the +2 oxidation state.
- In Cu₄O₄, copper is in the +1 oxidation state.
- In Cu₂P₄, copper is in the +2 oxidation state.

### Step 4: Calculate the Number of Electrons Transferred
For copper:
- Cu²⁺ (from Cu₂O₃ and Cu₂P₄) requires 2 electrons to deposit 1 mole of copper.
- Cu⁺ (from Cu₂Cl₂ and Cu₄O₄) requires 1 electron to deposit 1 mole of copper.

### Step 5: Calculate the Amount of Copper Deposited
Assuming we have 1 mole of each compound in 1 liter of solution:
- For Cu₂Cl₂ (1 mole):
- 1 mole of Cu⁺ will deposit 1 mole of Cu (1 electron).

- For Cu₂O₃ (1 mole):
- 1 mole of Cu²⁺ will deposit 0.5 mole of Cu (2 electrons).

- For Cu₄O₄ (1 mole):
- 1 mole of Cu⁺ will deposit 1 mole of Cu (1 electron).

- For Cu₂P₄ (1 mole):
- 1 mole of Cu²⁺ will deposit 0.5 mole of Cu (2 electrons).

### Step 6: Compare the Amounts of Copper Deposited
- Cu₂Cl₂: 1 mole of Cu deposited.
- Cu₂O₃: 0.5 mole of Cu deposited.
- Cu₄O₄: 1 mole of Cu deposited.
- Cu₂P₄: 0.5 mole of Cu deposited.

### Conclusion
The maximum amount of copper deposited by one Faraday current will be in the acidic solution of 1 liter of Cu₂Cl₂ or Cu₄O₄, both yielding 1 mole of copper.