Sample Exercise 5.12 Calculating an Enthalpy of Reaction from Enthalpies of Formation
{"Image DocumentName": "Sample Exercise 5.12 Calculating an Enthalpy of Reaction from Enthalpies of Formation", "Image ImageDescription": "Continued. Solve. (a) We know that a combustion reaction involves O2(g) as a reactant. Thus, the balanced equation or the combustion reaction of 1 mol C6H6(l) is C6H6(l) + O2(g) \u2192 6 CO2(g) + 3 H2O(l) We can calculate \u0394H \u00b0 for this reaction by using Equation 5.31 and data in Table 5.3. Remember to multiply the \u0394Hf \u00b0 value for each substance in the reaction by that substance\u2019s stoichiometric coefficient. Recall also that \u0394Hf \u00b0 = 0 for any element in its most stable form under standard conditions, so \u0394Hf \u00b0[O2(g)] = 0. \u2206H \u00b0rxn = [(6\u0394Hf \u00b0(CO2) + 3\u0394Hf \u00b0(H2O)] \u2013 [\u0394Hf \u00b0(C6H6) + \u0394Hf \u00b0(O2)] = [6(\u2212393.5 kJ) + 3(\u2212285.8 kJ)] \u2013 [(49.0 kJ) + (0 kJ)] = (\u22122361 \u2212 \u2212 49.0) kJ. = \u22123267 kJ.", "Image XResolution": "37", "Image YResolution": "37", "Image ResolutionUnit": "Pixels/Centimeter", "Image Software": "SlidePlayer", "Image YCbCrPositioning": "Centered"}