Consider the following standard electrode potentials ( $E^{o}$ in volts) in aqueous solution:
$\begin{matrix} \underset{}{E l e m e n t} & \underset{}{M^{3 +} / M} & \underset{}{M^{+} / M} \\ A l & - 1.66 & + 0.55 \\ T l & + 1.26 & - 0.34 \end{matrix}$
Based on these data, which of the following statements is correct?

Question

Consider the following standard electrode potentials (

E^{o}

in volts) in aqueous solution:

\begin{matrix} \underset{}{E l e m e n t} & \underset{}{M^{3 +} / M} & \underset{}{M^{+} / M} \\ A l & - 1.66 & + 0.55 \\ T l & + 1.26 & - 0.34 \end{matrix}

Based on these data, which of the following statements is correct?

Aicharya · Accepted Answer

&#8710; G o = - n F E o if E o = &#160; p o s i t i v e ; &#160; then &#8710; G o = n e g a t i v e , For those, conversions whose E o values are more positive are more favourable. As we can see from then electrode potential data, that reduction of Al + is spontaneous, but reduction of Tl + is not. So, we can conclude from this that T l + is more stable than A l +

Consider the following standard electrode potentials ( E o in volts) in aqueous solution: E l e m e n t M 3…

Solution