The Ni/Ni²⁺ and F/F₂ electrode potentials are listed as +0.25V and -2.87V respectively (with respect to the standard hydrogen electrode). The cell potential when these are coupled under standard conditions is:

• (A) 2.62V and dependent on the reference electrode chosen.
• (B) 3.12V and independent on the reference electrode chosen.
• (C) 3.12V and dependent on the reference electrode chosen.
• (D) 2.62V and independent of the reference electrode chosen.

To determine the cell potential when coupling the Ni/Ni²⁺ and F/F₂ half-reactions, we first need to calculate the overall cell potential using the given standard electrode potentials.

Electrode Potentials

The standard electrode potentials are:

• Ni/Ni²⁺: +0.25 V
• F/F₂: -2.87 V

Calculating the Cell Potential

The cell potential (E_cell) can be calculated using the formula:

E_cell = E_cathode - E_anode

In this case, fluorine (F/F₂) is the cathode (reduction) and nickel (Ni/Ni²⁺) is the anode (oxidation). Thus:

E_cell = (-2.87 V) - (+0.25 V) = -3.12 V

Interpreting the Result

Since we are looking for the absolute value of the cell potential, we take the positive value:

|E_cell| = 3.12 V

Reference Electrode Consideration

The cell potential is independent of the reference electrode chosen because standard electrode potentials are defined relative to the standard hydrogen electrode (SHE).

Final Answer

The correct option is (B) 3.12V and independent of the reference electrode chosen.