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For many substances, the formation reaction may be considered as the sum of a number of simpler reactions, either real or fictitious. The enthalpy of reaction can then be analyzed by applying Hess' law, which states that the sum of the enthalpy changes for a number of individual reaction steps equals the enthalpy change of the overall reaction.
It may provide or confirm basic enthalpy data needed for the calculation of phase diagrams of metals, via CALPHAD or ab initio quantum chemistry methods. For a binary system composed by elements A and B, a generic Miedema Formula could be cast as Δ H = f ( E l e m e n t A , P h i A , n W S A , V A , E l e m e n t B .
The enthalpy of formation of one mole of ethane gas refers to the reaction 2 C (graphite) + 3 H 2 (g) → C 2 H 6 (g). Standard enthalpy of hydrogenation is defined as the enthalpy change observed when one mole of an unsaturated compound reacts with an excess of hydrogen to become fully saturated.
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Std enthalpy change of formation, Δ f H o liquid: −597.0 kJ/mol Standard molar entropy, S o liquid? J/(mol K) Heat capacity, c p? J/(mol K) Gas properties Std enthalpy change of formation, Δ f H o gas: −592.0 kJ/mol Std Gibbs' free energy change of formation, Δ f G o gas: −545.2 kJ/mol Standard molar entropy, S o gas: 325 J/(mol K ...
Std enthalpy change of formation, Δ f H o solid: −1093.99 kJ/mol Standard molar entropy, S o solid: 88.7 J/(mol K) Heat capacity, c p? J/(mol K) Liquid properties Std enthalpy change of formation, Δ f H o liquid? kJ/mol Standard molar entropy, S o liquid? J/(mol K) Heat capacity, c p? J/(mol K) Gas properties Std enthalpy change of ...
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