Calculate the potential for a half cell reaction containing `0.1 M K_(2)Cr_(2)O_(7), 0.20 M Cr^(3+)(aq)` and `1.0xx10^(-4) M H^(+)(aq)`. The half cell reaction is :
`Cr_(2)O_(7)^(2-)(aq)+14 H^(+)(aq)+6e^(-)to2 Cr^(3+)(aq)+7H_(2)O (l)`
The standard electrode potential `(E^(@))=1.33 V`.

Explanation

To calculate the potential for the half-cell reaction given the concentrations of the reactants and the standard electrode potential, we will use the Nernst equation. Here’s a step-by-step solution:

### Step 1: Write the Nernst Equation
The Nernst equation is given by:
\[ E = E^\circ - \frac{0.0591}{n} \log Q \]
where:
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