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(c) This problem is rather time-consuming to solve without a computer program, and will therefore be left to the ambitious reader to solve59 from thermodynamic fundamentals. As an alternative, the reader may have access to tables that list heat of reaction information for important reactions. The following temperature-dependent heats of reaction were found for the water gas shift and reforming reactions in the Girdler tables (1). CH4 + H2O ⇔ 3H2 + CO ∆Hr(1800 oF)= 97,741 Btu/lb mol CO + H2O ⇔ CO2 + H2 ∆Hr(1800 oF)= -13,892 Btu/lb mol Note: a positive heat of reaction is endothermic (heat must be added to maintain a constant temperature), while a negative heat of reaction is exothermic (heat is given off). (d) With knowledge of the equilibrium concentration and the heats of reaction, the heat requirement for the reformer can be approximated. Knowing that for each lb mol of CH4 feed, 88.3 percent [(100-11.7)/100= 88.3 percent] of the CH4 was reformed, and 26.6 percent [23.5/88.3= 26.6 percent] of the formed carbon monoxide shifts to carbon dioxide, then the overall heat generation for each lb mol of methane feed can be developed from ⎛88.3% CH4 reacted⎞⎛ Btu ⎞ Btu (1 lbmol CH 4 )⎜⎝ 100% CH feed ⎟⎠ ⎜⎝ 97,741 lbmol reformed CH ⎟⎠ = 86,300 lbmol CH feed 444 ⎛ 88.3% CH rxtd. ⎞⎛ 1 lbmol CO ⎞⎛ 26.6% CO shifts ⎞⎛ - 13,982 Btu ⎞ ⎜ 4 ⎟⎜ ⎟ Btu lbmol CH (1lbmolCH ) ⎜ ⎟⎜ ⎟=-3,300 4 ⎜ 100% CH feed ⎟⎜ lbmol CH rxtd ⎟⎝ lbmol CO feed ⎠⎝ lbmol CO rxn ⎠ feed ⎝ 4 ⎠⎝ 4 ⎠ 4 Summing these results, the heat requirement for the reformer is about 83,000 Btu/lb mol of CH4 fed to the reformer. Because this value is positive, the overall reaction is endothermic and heat must be supplied. This approximate value neglects the change in sensible heat in taking the reactants from 1400 °F to the reference temperature of 1800 °F, and then the products from the reference temperature (1800 °F) back to 1400 °F. (e) LeChâtelier's Principle simply states that "if a stress is applied to a system at equilibrium, then the system readjusts, if possible, to reduce the stress". In this reforming example, LeChâtelier's Principle dictates whether higher or lower temperatures will promote the reforming reaction just by knowing that the reaction is endothermic. To facilitate the application of the principle, write the endothermic reforming reaction (which is the dominant heat of reaction) with a heat term on the left side of the equation. CH4 +H2O+Heat⇔3H2 +CO 59 The reader can refer to Reference 2, Example 4-8 for the solution of a related problem. 9-14PDF Image | Fuel Cell Handbook (Seventh Edition)
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