Calculate E_cell for the following electrochemical cell at 25 ^$\circ$C
Pt(s) | H₂(g,1.00 atm) | H⁺(aq,1.00 M) || Sn²⁺(aq,0.350 M) ,Sn⁴⁺(aq,0.020 M) | Pt(s)
Given the following standard reduction potentials.
Sn⁴⁺(aq) + 2 e^- $\to$ Sn²⁺(s) $~~~~~~~~$ E^$\circ$ = +0.15 V
2 H⁺(aq) + 2 e^- $\to$ H₂(g) $~~~~~~~~$ E^$\circ$ = 0.00 V

Question

Calculate E_cell for the following electrochemical cell at 25 ^$\circ$C
Pt(s) | H₂(g,1.00 atm) | H⁺(aq,1.00 M) || Sn²⁺(aq,0.350 M) ,Sn⁴⁺(aq,0.020 M) | Pt(s)
Given the following standard reduction potentials.
Sn⁴⁺(aq) + 2 e^-

\to

Sn²⁺(s)

~~~~~~~~

E^$\circ$ = +0.15 V
2 H⁺(aq) + 2 e^-

\to

H₂(g)

~~~~~~~~

E^$\circ$ = 0.00 V

Quizplus · Accepted Answer

The cell potential is calculated using the Nernst equation. The standard cell potential (E°cell) is 0.15 V - 0.00 V = 0.15 V. The reaction quotient Q = [Sn^4+]/[Sn^2+] = 0.020/0.350. Using the Nernst equation, Ecell = E°cell - (RT/nF)ln(Q), where n = 2, R = 8.314 J/mol·K, T = 298 K, and F = 96485 C/mol. This gives Ecell ≈ 0.11 V.

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

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