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Chapter 3. Sustainable Hydrocarbon Fuels by Recycling CO2 with Renewable/Nuclear Energy 52 estimated from as high as $100-200 per tonne of CO2 (tCO2) [40, 51] to a long term cost as low as $30/tCO2 [2] for this new method. 3.2.2. Dissociation of H2O and CO2 Dissociation of H2O, CO2, or mixtures of both is the stage with the largest energy conversion, because this is where the energy is stored as fuel or fuel precursors. The minimum required energy is the enthalpy of the reactions: H2O H2 + 1⁄2 O2 = 286 kJ/mol CO2 CO + 1⁄2 O2 = 283 kJ/mol Electrical energy can be used to drive the dissociations via electrolysis. However, heat can generally be obtained at a lower cost than electricity. For example, converting solar energy to heat can theoretically be carried out more efficiently and more inexpensively than photovoltaic (PV) conversion to electricity, which suggests that splitting water in solar furnaces should be preferred over the electrolytic splitting of water. However, using heat for dissociation is a more difficult process, requiring expensive materials that are stable at very high temperature (for thermolysis) or requiring a complicated multiple-step process that needs careful materials handling and heat management at each step (for thermochemical cycles), as will be discussed further in the following sections. H2O dissociation for H2 production has been much more widely researched than CO2 dissociation. Rather than disassociating the CO2 directly, hydrogen may be used to reduce CO2 to CO via the reverse water-gas shift (RWGS) reaction, RWGS WGS The same reactants may be used with different conditions and catalysts in hydrogenation reactions to directly produce fuels such as methanol – these have been the most studied reactions in CO2-recycled synthetic fuel research and will be discussed further in section 3.2.3. Alternatively, CO2 can be dissociated instead, and the resulting CO used to reduce H2O to H2 in the water-gas shift (WGS) reaction. Figure 3-4 shows the thermodynamics of the dissociation and WGS reactions. In some cases, splitting CO2 may have advantages. For example, when the reactant (H2O or CO2) should be gaseous, water requires vaporization to steam whereas room temperature CO2 is already a gas and can be used directly. On the other hand, if low temperature heat (>100 °C) is available to produce steam, the energy consumption of the actual dissociation can be reduced to 249 kJ/mol. Finally, separating the products from unconverted reactants may be easier with H2/H2O because the H2O can simply be condensed to liquid, whereas CO/CO2 would require gas phase separation. H2 + CO2 H2O + COPDF Image | Electrolysis of CO2 and H2O
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