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

\rightarrow

2Ag(s) + 2H⁺(aq) + 2C^-(aq)

Quizplus · Accepted Answer

The equilibrium constant (K) for a reaction can be calculated using the Nernst equation or its derived form, which relates the standard cell potential ($E^0$) to the equilibrium constant. The formula is $E^0 = \frac{0.0592}{n} \log K$, where $n$ is the number of electrons transferred in the reaction. Given $E^0 = +0.22$ V and assuming $n = 2$ for the reduction of Ag$^+$ to Ag (as implied by the reaction), solving for $K$ gives a value in the range of $10^{7}$, which corresponds to the option indicating $2.7 \times 10^{17}$.

The Standard Voltage of the Cell Pt|H2(g)|H+(aq)M Cl-(aq)|AgCl(s)|Ag(s) Is +0 ο\omicronο

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