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One mole of particles given 1 eV of energy each has approximately 96.5 kJ of energy – this corresponds to the Faraday constant (F ≈ 96 485 C⋅mol −1), where the energy in joules of n moles of particles each with energy E eV is equal to E·F·n.
11 Αυγ 2013 · It means that per mole water splitting requires at least $241.8\ \mathrm{kJ}$ of energy. Any method(thermal,electrolysis etc) followed, this much of energy will be always required. When using electrolysis, it may be convenient to express it in $\mathrm{eV}$.
13 Φεβ 2023 · The activation energy (Ea), labeled ΔG ‡ in Figure 2, is the energy difference between the reactants and the activated complex, also known as transition state. In a chemical reaction, the transition state is defined as the highest-energy state of the system.
Quite often (eg in thermal desorption spectroscopy) energies like activation or desorption energy are stated in either electron volt or kJ/mol.
7 Δεκ 2023 · 1 eV = 1.6 × 10 –19 J In order to convert between electronvolts and joules: Multiply electronvolts by 1.6 × 10 –19 to get the equivalent energy in joules
The chemical formula of water is H 2O. Its molecu-lar structure is roughly as shown below: The density of water, at standard temperature and pressure is, by definition ρ = 1 gm ⁄ cm3 = 103 kg ⁄ m3. Since the molecular weight of water (ignoring isotopes like 18O and 2H) is 18, the number density of molecules in liquid water is n = NA 18 ≈ ...
The 237kJ/mol is the Gibbs free energy required for electrolysis, while the 286kJ/mol normally quoted for combustion is the enthalpy. To compare the two you need to take into account heat exchange with the environment and even the work done by the escaping gas.
