For the electrochemical cell $\begin{aligned} ext{If } E_{(M^{2+}/M)}^0=0.46 ext{ V and } E_{(x/X^{2-})}^0=0.34 ext{ V.} \end{aligned}$ Which of the following is correct?

Question

For the electrochemical cell $\begin{aligned} 	ext{If } E_{(M^{2+}/M)}^0=0.46 	ext{ V and } E_{(x/X^{2-})}^0=0.34 	ext{ V.} \end{aligned}$ Which of the following is correct?

Aicharya · Accepted Answer

$\begin{aligned} & \mathrm{M} \mid \mathrm{M}^{+2} \| \mathrm{X} / \mathrm{X}^{2-} \\ & \mathrm{E}_{\mathrm{cell}}^{\mathrm{o}}=\mathrm{E}_{\mathrm{M} / \mathrm{M}^{+2}}^{\mathrm{o}}+\mathrm{E}_{\mathrm{X} / \mathrm{X}^{-2}}^{\mathrm{o}} \\ & =-0.46+0.34=-0.12 \mathrm{~V} \end{aligned}$
As $\mathrm{E}_{\text {cell }}^{\mathrm{o}}$ is negative so anode becomes cathode and cathode become anode. Spontaneous reaction will be $\mathrm{M}^{+2}+\mathrm{X}^{2-} \longrightarrow \mathrm{M}+\mathrm{X}$

For the electrochemical cell $\begin{aligned} \text{If } E_{(M^{2+}/M)}^0=0.46 \text{ V and }…

Solution