Question

For the electrochemical cell, $\left(M|M^{\oplus }\right)||\left(X^{\ominus }|X\right),E_{\left(M^{\oplus }|M\right)}^{\ominus }=0.44V,$ and $E_{\left(x|X^{\ominus }\right)}^{\ominus }=-0.33V$. From this data, one can conclude that:

• A. $M+X\to M^{\oplus }+X^{\ominus }$ is the spontaneous reaction
• B. $M^{\oplus }+X^{\ominus }\to M+X$ is the spontaneous reaction
• C. $E_{cell}^{\ominus }=0.77V$
• D. $E_{Cell}^{\ominus }=-0.77V$

Answer 1

Answer: (B), (C)

$E_{cell}^{\ominus }=0.77V$
$M^{\oplus }+X^{\ominus }\to M+X$ is the spontaneous reaction

$E-cell=E_{oxidation}-E_{reduction}$

Spontaneous reaction : $M^{\oplus }+X^{\ominus }\to M+X$

because $E_{cell}^{\ominus }=0.44-(-0.33)=0.77V>0$