Skip to main content
Chemistry

Return to Answer

Formatted the values with MathJax. Also, there’s no need for your excessive bolding and italicising.
Source Link
Jan
Jan
  • 68.7k
  • 12
  • 205
  • 389

With Standardthe standard electrode potential assumed to be -0.358 V$\pu{-0.358 V}$, I am getting the same answer as you but I googled out for the standard electrode potential of the above reaction and I found it to be -0.320 V$\pu{-0.320 V}$. On substituting -0.320 V$\pu{-0.320 V}$ as the standard electrode potential, I got -0.529 V$\pu{-0.529 V}$.

With Standard electrode potential assumed to -0.358 V, I am getting the same answer as you but I googled out for the standard electrode potential of the above reaction and I found it to be -0.320 V. On substituting -0.320 V as the standard electrode potential, I got -0.529 V.

With the standard electrode potential assumed to be $\pu{-0.358 V}$, I am getting the same answer as you but I googled the standard electrode potential of the above reaction and I found it to be $\pu{-0.320 V}$. On substituting $\pu{-0.320 V}$ as the standard electrode potential, I got $\pu{-0.529 V}$.

Source Link
Yb609
Yb609
  • 1.7k
  • 12
  • 21

With Standard electrode potential assumed to -0.358 V, I am getting the same answer as you but I googled out for the standard electrode potential of the above reaction and I found it to be -0.320 V. On substituting -0.320 V as the standard electrode potential, I got -0.529 V.