The standard voltage of the cell Pt|H₂(g) |H⁺(aq) m Cl^-(aq) |AgCl(s) |Ag(s)
Is +0.22 V at 25^$\circ$C.Calculate the equilibrium constant for the reaction below.
2AgCl(s) + H₂(g) $\rightarrow$ 2Ag(s) + 2H⁺(aq) + 2Cl^-(aq)

Question

The standard voltage of the cell Pt|H₂(g) |H⁺(aq) m Cl^-(aq) |AgCl(s) |Ag(s)
Is +0.22 V at 25^$\circ$C.Calculate the equilibrium constant for the reaction below.
2AgCl(s) + H₂(g)

\rightarrow

2Ag(s) + 2H⁺(aq) + 2Cl^-(aq)

Quizplus · Accepted Answer

The equilibrium constant (K) can be calculated using the Nernst equation: E° = (RT/nF)lnK. Given E° = +0.22 V, n = 2, R = 8.314 J/mol·K, T = 298 K, and F = 96485 C/mol, solving for K gives approximately 2.7 * 10^7.

The Standard Voltage of the Cell Pt|H2(g)|H+(aq)m Cl-(aq)|AgCl(s)|Ag(s) Is +0 ∘\circ∘

The Standard Voltage of the Cell Pt|H₂(g)|H⁺(aq)m Cl^-(aq)|AgCl(s)|Ag(s)
Is +0 $\circ$