Which graph correctly correlates Ecell as a function of concentrations for the cell Zn(s)+2 Ag^

step 1 According to NUst equations, I can write a expression as E -shell is equal to E -shell -0 minus

Which graph correctly correlates Ecell as a function of...

Which graph correctly correlates $E_{\text {cell }}$ as a function of concentrations for the cell $$ \mathrm{Zn}(s)+2 \mathrm{Ag}^{+}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+2 \mathrm{Ag}(s), \quad E_{\text {cell }}^{\circ}=1.56 \mathrm{~V} $$ $Y$ -axis : $E_{\text {cell }}, X$ -axis : $\log _{10} \frac{\left[\mathrm{Zn}^{2+}\right]}{\left[\mathrm{Ag}^{+}\right]}$

Which graph correctly correlates $E_{\text {cell }}$ as a function of concentrations for the cell
$$
\mathrm{Zn}(s)+2 \mathrm{Ag}^{+}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+2 \mathrm{Ag}(s), \quad E_{\text {cell }}^{\circ}=1.56 \mathrm{~V}
$$
$Y$ -axis : $E_{\text {cell }}, X$ -axis : $\log _{10} \frac{\left[\mathrm{Zn}^{2+}\right]}{\left[\mathrm{Ag}^{+}\right]}$

Key Concepts

Nernst Equation

The Nernst equation relates the cell potential to the reaction quotient and allows us to calculate how the potential deviates from its standard value as the concentrations of reactants and products change. It is given by E = E° - (RT/nF) ln Q, where E° is the standard cell potential, R is the gas constant, T the temperature, n the number of electrons transferred, F the Faraday constant, and Q the reaction quotient. This equation is pivotal for understanding the dependence of cell potential on the logarithm of concentration ratios.

Reaction Quotient (Q)

The reaction quotient is a dimensionless number that represents the ratio of the concentrations (or activities) of products to those of reactants, each raised to the power of their respective stoichiometric coefficients. In electrochemical cells, Q appears in the Nernst equation and quantifies the shift in equilibrium from standard conditions. It is essential for determining how concentration changes influence the cell potential.

Logarithmic Transformation in Electrochemistry

Because the Nernst equation involves a logarithmic term, the relationship between the cell potential and the concentration ratio becomes linear when plotted against the logarithm of this ratio. Converting the natural logarithm to a common logarithm (using the factor 2.303) simplifies the graphical interpretation, making it easier to correlate changes in concentration with shifts in the cell potential.

Electrochemical Cell Potential

The electrochemical cell potential (or electromotive force) is the measure of the energy available from the redox reaction in an electrochemical cell. It is determined by the difference between the potentials of the two electrodes, and its dependence on concentration is captured by the Nernst equation. Understanding this potential is crucial for analyzing the efficiency and direction of redox reactions in various electrochemical applications.

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