8. Bonus ( 10 points) Take a generic balanced oxidation/reduction reaction of two metals at \( 25^{\circ} \mathrm{C} \) : \[ 3 \mathrm{~A}^{0}+2 \mathrm{~B}^{+3} \rightarrow 3 \mathrm{~A}^{2+}+2 \mathrm{~B}^{\circ} \] If the Gibb's free energy for this battery was \( -265 \mathrm{KJ} / \) mole, calculate \( \mathrm{E} \) for this reaction if the concentration of \( \mathrm{B}^{+3} \) is \( .36 \mathrm{M} \) and \( \mathrm{A}^{2+} \) is \( .4 \mathrm{M} \).
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From the balanced equation, we can see that the number of moles of electrons transferred in the reaction is 6 (3 from each A atom). So, we can rearrange the equation to solve for E: E = -ΔG / (nF) Substituting the given values: E = -(-265,000 J/mol) / (6 mol Show more…
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