Calculate E_cell for the following electrochemical cell at 25 ^$\circ$C
Pt(s) | Fe³⁺(aq,0.100 M) ,Fe²⁺(aq,0.040 M) || Cl^-(aq,0.50 M) | AgCl(s) | Ag(s)
Given the following standard reduction potentials.
AgCl(s) + e^- $\to$ Ag(s) + Cl^-(aq) $~~~~~~~~$ E^$\circ$ = +0.222 V
Fe³⁺(aq) + e^- $\to$ Fe²⁺(aq) $~~~~~~~~$ $~~~~~~~~$ E^$\circ$ = +0.771 V

Question

Calculate E_cell for the following electrochemical cell at 25 ^$\circ$C
Pt(s) | Fe³⁺(aq,0.100 M) ,Fe²⁺(aq,0.040 M) || Cl^-(aq,0.50 M) | AgCl(s) | Ag(s)
Given the following standard reduction potentials.
AgCl(s) + e^-

\to

Ag(s) + Cl^-(aq)

~~~~~~~~

E^$\circ$ = +0.222 V
Fe³⁺(aq) + e^-

\to

Fe²⁺(aq)

~~~~~~~~

~~~~~~~~

E^$\circ$ = +0.771 V

Quizplus · Accepted Answer

To calculate the cell potential, we need to subtract the reduction potential of the anode (Fe3+ reduction) from the reduction potential of the cathode (AgCl reduction). Ecell = Ered^cathode - Ered^anode Ecell = +0.222 V - (+0.771 V) Ecell = -0.549 V Since the anode is on the left side of the cathode in the cell notation, we need to flip the sign of the cell potential to get the standard cell potential (E_cell). E_cell = -Ecell E_cell = -(-0.549 V) E_cell = +0.549 V Therefore, the best choice is D) -0.555 V, which is closest to the calculated value of +0.549 V (rounded to three significant figures).

Calculate Ecell for the Following Electrochemical Cell at 25 ∘\circ∘

Calculate E_cell for the Following Electrochemical Cell at 25 ^$\circ$