Consider the following `E^(@)` values `E^(@)` values `E_(Fe^(3+)//Fe^(2+))^(@)= 0.77v` , `E_(Sn^(2+)//Sn)^(@) = -0.14` under standard condition the potential for the reaction `Sn_(s)+ 2Fe^(3+)(aq)rightarrow 2Fe^(2+)(aq) + Sn^(2+) (aq)` is :

Options

A. (1.68V)
B. (0.63V)
C. (0.91V)
D. (1.40V)

Explanation

To find the standard cell potential (E°cell) for the reaction:

\[ \text{Sn}_{(s)} + 2\text{Fe}^{3+}_{(aq)} \rightarrow 2\text{Fe}^{2+}_{(aq)} + \text{Sn}^{2+}_{(aq)} \]

we will follow these steps:

### Step 1: Identify the half-reactions
The given half-reactions based on the standard electrode potentials are:
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