96485kJmol

96485 kJ mol⁻¹ is a numerical value that appears in the field of electrochemical thermodynamics. The number is derived from the product of Avogadro’s number, the elementary charge, and the units conversion between joules and volts. In practice, the Faraday constant is normally expressed in coulombs per mole, F ≈ 96485 C mol⁻¹. When the energy equivalent of a single coulomb of charge is taken as one joule per volt, the Faraday constant can be expressed in energy units: 96485 J mol⁻¹, which is equivalent to 96.485 kJ mol⁻¹. The higher figure of 96485 kJ mol⁻¹ is sometimes presented erroneously in literature, but it would correspond to the energy conversion for a charge transported through a potential difference of 1000 V rather than the standard 1 V.

The 96.485 kJ mol⁻¹ value is widely used to relate electrical work to Gibbs free‑energy changes in redox reactions through the equation ΔG = - n F ΔE, where ΔE is the electrode potential in volts and n is the number of electrons transferred. This relation underpins the Nernst equation and the calculation of standard electrode potentials. In battery science, electrolysis, and corrosion studies, the Faraday constant in energy form provides a convenient bridge between electrical measurements and thermodynamic quantities. The value is temperature dependent only slightly; at 298 K the accepted value is 96.485 kJ mol⁻¹, and it is documented in multiple reference works such as the NIST Chemistry WebBook and the International Union of Pure and Applied Chemistry (IUPAC) recommendations.