Consider the following cell reaction: `2Fe(s)+O_(2) (g) + 4H^(+)(aq)to2Fe^(2+)(aq)+2H_(2)O(l)`, `E^(@) = 1.67V`
At `[Fe^(2+)] = 10^(-3)M,P_(O_2)=0.1` atm and PH=3 . The cell potential at `25^(@) C`:

Options

A. `(1.47V)`
B. `(1.77V)`
C. `(1.87V)`
D. `(1.57V)`

Explanation

To calculate the cell potential at the given conditions, we will use the Nernst equation. The Nernst equation relates the cell potential under non-standard conditions to the standard cell potential and the concentrations of the reactants and products involved in the reaction.

### Step-by-Step Solution:

1. **Identify the Standard Cell Potential (E°)**:
The standard cell potential (E°) is given as 1.67 V.

2. **Determine the Reaction**:
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