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By Daniel A Murray
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A large discrepancy amounting to 1520 % of the total energy input appears. This can be partially explained by the following. It is difficult and sometimes impossible to determine the enthalpies of all the substances produced in metallurgical and chemical processes, as the reference books have no values of L1H for slags, mattes and similar materials whose composition may be very complex or unknown. In addition the enthalpies of formation of these substances are usually considerably higher than the values of L1H of the initial fuel, raw material, fluxes, etc.
4) where (L1H~)aq and (L1G~)aq are the enthalpy and free enthalpy (the Gibbs energy) of formation of a substance in aqueous solution, respectively. 3,4) allow one to determine the values of the chemical energy and exergy of an element when these values are known for all the other elements of the considered substance. g. [43, 126, 128], can also be used to calculate the chemical energy and exergy of substances. These potentials are determined experimentally with respect to some reference standard, usually a hydrogen electrode under standard conditions.
H2. , the standard electrode potential of this reaction, is set equal to zero. In our technique, however, the chemical energy and exergy of water and oxygen, rather than hydrogen potentials, are taken as the zero level. ; H20. 34 kJ/mole. 23 V , which is the resulting potential of a hydrogen electrode. , e~2 =- (LlG~20) and i~2 =- (LlG~20) . tn The essence of the procedure of changing the reference level is illustrated Fig. 1. It shows the potentials of some metals relative to the zero (standard) potential of reaction of hydrogen ion formation.
An elementary course in the integral calculus by Daniel A Murray