Industry generates to the atmosphere greater and greater amounts of CO(2)harmful to
the environment. Its use as a raw material in the production of synthetic fuels realizes
the idea of 'Clean Production', in which products are made is a sustainable environment
conditions. A chemical model was created using an innovative chemical process of CO(2)and
H(2)synthesis. A thermodynamic analysis of such a process was carried out, determining
energy barriers and favourable conditions for its course. This model's process comprises
reactions representing three of its stages :1) synthesis of methanol (METH) and dimethyl
ether (DME) with CO(2)and H-2, 2) conversion of the mixture of methanol, ether and
water into light olefins and 3) hydrogenation of olefins (C-2-C-6) to the mixture
of paraffins - gasoline. Calculations were made for changes for enthalpy and Gibbs
free energy of respective reactions for each stage. The analysis showed that at no
stage of the process the level of energy barrier does not exclude (in terms of technology)
the possibility of the execution of the process. The equilibrium conversion of CO(2)within
the temperature range (T): = 475-575 K, for p = 1 MPa, and H-2/CO2 = 3/1 remains within
20-25%, at products selectivity DME/METH/CO = 0.73/0.14/0.17, at 475 K and 0.0038/0.013/0.98
at 573 K. Olefins are produced in exothermic reactions of DME and METH conversion
and the changes in their yield with temperature run through maximum values, which
along with increase of carbons in the olefin are shifted towards lower temperatures.
Thermal effects Delta H) of the olefin hydrogenation reaction are similar and are
their values range between (-124) and (-137) KJ/mol. Thermodynamic limitations for
these reactions no longer exist for temperature <950 K, and their lower conversion
at higher temperature can be compensated with increase in pressure (Chatelier's principle).
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