How do you calculate the electrode potential under nonstandard conditions using the Nernst equation?

• A. E = E° + (nF/RT) ln(Q)
• B. E = E° + (RT/nF) ln(Q)
• C. E = E° - (nF/RT) ln(Q)
• D. E = E° - (RT/nF) ln(Q)

Answer: (D)

Verified step by step guidance

1. Identify the correct form of the Nernst equation for calculating electrode potential under nonstandard conditions. The correct form is: $E=E_{°}-\left(\frac{RT}{nF}\right)\ln \left(Q\right)$
2. Understand the components of the Nernst equation: $E_{°}$ is the standard electrode potential, $R$ is the universal gas constant (8.314 J/mol·K), $T$ is the temperature in Kelvin, $n$ is the number of moles of electrons transferred, $F$ is Faraday's constant (96485 C/mol), and $Q$ is the reaction quotient.
3. Convert the temperature to Kelvin if it is given in another unit, such as Celsius. Use the conversion formula: $T=\mathrm{°C}+273.15$
4. Calculate the reaction quotient $Q$ using the concentrations or partial pressures of the reactants and products involved in the electrochemical reaction. The expression for $Q$ is typically the ratio of the product concentrations raised to their stoichiometric coefficients divided by the reactant concentrations raised to their stoichiometric coefficients.
5. Substitute the values of $E_{°}$, $R$, $T$, $n$, $F$, and $Q$ into the Nernst equation to calculate the electrode potential $E$ under nonstandard conditions.