Standard electrode potential for the cell with cell reaction $\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(\mathrm{aq}) \longrightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Cu}(\mathrm{s})$ is $1.1 \mathrm{~V}$. Calculate the standard gibbs energy change for the cell reaction. (Given $\mathrm{F}=96487 \mathrm{C} \mathrm{mol}^{-1}$ )

• A

  $-200.27 \mathrm{~kJ} \mathrm{~mol}^{-1}$
• Correct answer
  B

  $-212.27 \mathrm{~kJ} \mathrm{~mol}-1$
• C

  $-212.27 \mathrm{~J} \mathrm{~mol}^{-1}$
• D

  $-200.27 \mathrm{~J} \mathrm{~mol}^{-1}$

Hence, the correct answer is option: 'B'.