Read the passage carefully and answer.

When a metal is placed in a solution of its ions, the metal can lose electron and can go in the solution as ion or the metal ion in the solution can take electron from the electrode and get deposited as metal. Thus, the electrode acquires either positive or negative charge with respect to the solution leading to the development of a potential difference between the metal electrode and the solution. This potential difference is called the electrode potential of the metal. The electrode potential of a metal is a measure of relative tendency to undergo oxidation (loss of electron) or reduction (gain of electron). When the concentration of the ions in the solution is unity, the electrode potential is called standard electrode potential. The magnitude of potential depends upon the nature of electrode, concentration of ions in solution and the temperature. In a galvanic cell, the electrode at which oxidation occurs is known as anodic half-cell and the electrode at which reduction occurs is known as cathodic half cell. The emf of the cell in terms of standard reduction potential is given by $E°_{cell} = E°_{cathode} - E°_{anode}$. The standard free energy change of the redox reaction taking place in the cell is related to $E°_{cell}$ by $ΔG°= -nFE°$. A redox reaction would occur spontaneously if the free energy change is negative. The equilibrium constant of the reaction is related to the standard free energy change by $ΔG°= -RT$ In K.

The equilibrium constant of a feasible cell reaction is

greater than one

The correct answer is Option (2) → greater than one

Based on the passage and the principles of electrochemistry, the correct answer is greater than one.

Here is the step-by-step breakdown of why this is the case:

1. The Condition for Feasibility

The passage states that a redox reaction occurs spontaneously (is "feasible") if the free energy change (ΔG°) is negative. 

2. The Relationship Between ΔG° and K

The passage provides the equation relating standard free energy to the equilibrium constant (K): 

$ΔG° = \text{−RT ln K}$

3. Mathematical Analysis

To make AG° a negative value (which is required for a feasible reaction):

• R (gas constant) and T (temperature in Kelvin) are always positive.
• Therefore, the term In K must be positive.
• For the natural logarithm of a number to be positive ($\text{ln K > 0}$), the number K must be greater than 1.