Calculate the oxidation potential of a hydrogen electrode at ph =1(T=298k)?

Question

Answer

Calculation of Oxidation Potential of a Hydrogen Electrode at pH = 1 (T = 298 K)

In order to calculate the oxidation potential of a hydrogen electrode at pH = 1 and a temperature of 298 K, we need to consider the Nernst equation, which relates the electrode potential to the concentration of species involved in the redox reaction.

Nernst Equation:

The Nernst equation is given by:

E = E0 - (RT/nF) * ln(Q)

Where:

E is the electrode potential

E0 is the standard electrode potential

R is the gas constant (8.314 J/(mol·K))

T is the temperature in Kelvin

n is the number of electrons transferred in the redox reaction

F is the Faraday constant (96485 C/mol)

Q is the reaction quotient, which is the ratio of product concentrations to reactant concentrations

Determination of E0:

The standard electrode potential, E0, for a hydrogen electrode is 0 V at standard conditions (25°C, 1 atm pressure, and a pH of 0). However, at pH = 1, the hydrogen electrode potential is slightly different due to the change in pH.

The Nernst equation can be rearranged as:

E = E0 - (2.303RT/nF) * pH

For the hydrogen electrode, n is equal to 2, as two electrons are involved in the redox reaction.

Calculating the Oxidation Potential:

Given pH = 1 and T = 298 K, we can substitute these values into the equation:

E = 0 V - (2.303 * 8.314 J/(mol·K) / (2 * 96485 C/mol)) * (298 K) * (1)

Simplifying the equation:

E = -0.059 V

Conclusion:

The oxidation potential of a hydrogen electrode at pH = 1 and T = 298 K is approximately -0.059 V. This value indicates that the hydrogen electrode is under oxidizing conditions at this pH and temperature.

Answer

E=.0591

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