The quinhydrone half cell is represented as Pt / H2 Q, Q, H^+(aq). H2 Q and Q are present in 1:

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The quinhydrone half cell is represented as Pt / H2 Q, Q,...

The quinhydrone half cell is represented as $\mathrm{Pt} / \mathrm{H}_2 \mathrm{Q}, \mathrm{Q}$, $\mathrm{H}^{+}(\mathrm{aq})$. $\mathrm{H}_2 \mathrm{Q}$ and Q are present in $1: 1$ molar ratio. The electrode potential of the above electrode is written as (a) $\mathrm{E}=\mathrm{E}^{\circ}+0.059 \log \left[\mathrm{H}^{\prime}\right]$ (b) $\mathrm{E}=\mathrm{E}^{\bullet}-0.059 \log \left[\mathrm{H}^{-}\right]$ (c) $\mathrm{E}=\mathrm{E}^{\circ}-\frac{0.059}{2} \log \left(\frac{\mathrm{H}_2 \mathrm{Q}}{\mathrm{Q}}\right)$ (d) $\mathrm{E}=\mathrm{E} 0+\frac{0.059}{2} \log \left(\frac{[\mathrm{Q}]\left[\mathrm{H}^{+}\right]}{\left[\mathrm{H}_2 \mathrm{Q}\right]}\right)$

The quinhydrone half cell is represented as $\mathrm{Pt} / \mathrm{H}_2 \mathrm{Q}, \mathrm{Q}$, $\mathrm{H}^{+}(\mathrm{aq})$.
$\mathrm{H}_2 \mathrm{Q}$ and Q are present in $1: 1$ molar ratio. The electrode potential of the above electrode is written as
(a) $\mathrm{E}=\mathrm{E}^{\circ}+0.059 \log \left[\mathrm{H}^{\prime}\right]$
(b) $\mathrm{E}=\mathrm{E}^{\bullet}-0.059 \log \left[\mathrm{H}^{-}\right]$
(c) $\mathrm{E}=\mathrm{E}^{\circ}-\frac{0.059}{2} \log \left(\frac{\mathrm{H}_2 \mathrm{Q}}{\mathrm{Q}}\right)$
(d) $\mathrm{E}=\mathrm{E} 0+\frac{0.059}{2} \log \left(\frac{[\mathrm{Q}]\left[\mathrm{H}^{+}\right]}{\left[\mathrm{H}_2 \mathrm{Q}\right]}\right)$

Key Concepts

Electrode Potential

The electrode potential is a measure of the energy change associated with the transfer of electrons from one species to another at an electrode interface. It reflects the driving force behind redox reactions in an electrochemical cell and is defined relative to a standard reference, providing insight into the tendency of a species to undergo oxidation or reduction.

Nernst Equation

The Nernst equation is a fundamental relation in electrochemistry that connects the electrode potential of a half-cell to the standard electrode potential, temperature, number of electrons involved in the redox process, and the activities or concentrations of the chemical species in equilibrium. It allows for the calculation of potential under non-standard conditions by accounting for changes in species activity.

Redox Equilibrium

Redox equilibrium describes the state in which the rates of oxidation and reduction are balanced within a system, resulting in constant concentrations of the oxidized and reduced species. This concept is crucial for understanding how changes in species concentrations, as described by the Nernst equation, affect the overall potential of an electrochemical cell.

Half-Cell Representation

A half-cell in electrochemistry denotes the region where either oxidation or reduction occurs. It is typically represented by a notation that includes the electrode material and the reactants/products involved in the redox reaction. This representation is essential for applying the Nernst equation and analyzing the components of an electrochemical cell.

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