Question

For a certain redox reaction, $E ^{0}$ is positive. This means that:

• A. $\Delta G^{0}$ is positive, $K_{\text {eqm }}$ is greater than 1
• B. $\Delta G^{0}$ is positive, $K_{\text {eqm }}$ is less than 1
• C. $\Delta G^{0}$ is negative, $K_{\text {eqm }}$ is greater than 1
• D. $\Delta G^{0}$ is negative, $K_{\text {eqm }}^{c_{m}}$ is less than 1

Answer 1

Answer: (C)

$\Delta G ^{0}=- nFE ^{0}.......(i)$

$\Delta G^{0}=-2.303 RT \log K _{ eq}.....(ii)$

From eq (i) if $E ^{0}$ is positive

then $\Delta G ^{0}$ is negative In equation (ii), $\Delta G^{0}$ is negative

So; $\log K >0 \Rightarrow K >1$