Question

The following reaction takes place in a galvanic cell at \(298\) K \[ \mathrm{Fe^{2+}(aq)+Ag^+(aq)\rightarrow Fe^{3+}(aq)+Ag(s)} \] The \(\Delta_rG^\circ\) (in kJ mol\(^{-1}\)) and \(\log K_c\) values are respectively \[ (F=96500\ \mathrm{C\,mol^{-1}},\; E^\circ_{\mathrm{Ag^+/Ag}}=0.80\ \mathrm{V},\; E^\circ_{\mathrm{Fe^{3+}/Fe^{2+}}}=0.77\ \mathrm{V},\; R=8.3\ \mathrm{J\,mol^{-1}K^{-1}}) \]

• A. \(-0.508;\ 2.895\)
• B. \(2.895;\ 5.08\)
• C. \(-2.895;\ 0.508\)
• D. \(2.895;\ 0.508\)

Hint:

Remember, \[ \boxed{ \Delta G^\circ=-nFE^\circ_{\text{cell}} } \] and \[ \boxed{ \Delta G^\circ=-2.303RT\log K. } \]

Answer 1

The Correct Option is C