\fin k], kJ and UK respectively, per 1 gram ofglucose. Glucose's molecular weight is 180.16 9. Other thermodynamic quantities change as well between the reactants and the products. Compute, per 1 g of glucose, the change in constant pressure heat capacity, ACP. Use the values in the table, even for gases (the equipartition theorem answer is not particularly accurate for carbon dioxide). Do the calculation at room temperature (298K) and don't round! We will need these numbers for the other questions, so keep them accurate (1% accurary required). AG: u AH: kJ AS = UK (Hint: Is it more accurate to compute AS as (AH AG)/T, or directly from the table?) A013: .J/K Reference Data Thermodynamic Properties of Selected Substances All of the values in this table are for one mole of material at 298 K and 1 bar. Following the chemical formula is the form of the substance, either solid (3), liquid (1), gas (g), or aqueous solution (aq) When there is more than one common solid form, the mineral name or crystal structure is indicated. Data for aqueous solutions are at a standard concentration of 1 mole per kilogram water. The enthalpy and Gibbs free energy of formation, AIH and fG, represent the changes in H and G upon forming one mole of the material starting with elements in their most stable pure states (e.g., C (graphite), 02 (g), etc). To obtain the value of AH or AG for another reaction, subtract A; of the reactants from AI of the products. For ions in solution there is an ambiguity in dividing thermodynamic quantities between the positive and negative ions; by convention, H+ is aSSiEIled the value zero and all others are chosen to be consistent with this value. Data from Atkins (1998), Lide (1994), and Anderson (1996). Please note that, while these data are sufficiently accurate and consistent for the examples and problems in this textbook, not all of the digits shown are necessarily signicant; for research purposes you should always consult original literature to determine experimental uncertainties. . "'l""""'}* l'" . 3' ....... 3.----_. -l----- - n. _,_____.,__ ""3"\" .- .v-..- 27' Other thermodynamic quantities change as well between the reactants and the products. Compute. per 1 g of glucose, the change in constant pressure heat capacity, ACp. Use the values in the table, even for gases (the equipartition theorem answer is not particularly accurate for carbon dioxide). Do the calculation at room temperature (298K) and don't round! We will need these numbers for the other questions, so keep them accurate (1% accurary required). AG = -2878.94 a k] AH = 2303.04 E U AS = 254.70 E J/K (Hint: Is it more accurate to compute AS as (AH AG)/T, or directly from the table?) A012: 383.12 E J/K 1 5. 55 X10-3 moles n moles C6 Hi2 06 = 180 AG = 2 Gproduct - & Greactant ( 6 Geo2 + 6 GM20) - ( GCCH120 + 6 6 Groz) =[(6(-294 36) + 6(-237.13 )) - (- 910 + 6 (0)) In = - 28 78 94 X 5. 5506 X10-3) 15. 9798 AH = 2 Hproduct - 2 Hreactant = 6 Hcoz + 6HMO) - (HGH1206 + * 6 Ho2 )In = [6(-393.51) + 6( - 285.83)) - (-1273) 75.5 5 710-2 15.5568 K J AS = AS product - 45 reactant = [(6(213- 74) + 6 (69. 91)) - (212 + 6 * 205.14) n 1. 4377 J/K ACp = ( CP ) products ( CP ) reactant = [(6 ( 37.11) + 6 ( 75. 29)) - ( 115 + 6(29.38)) ( 5:55 x109 2. 126 J /K