5. (40 pts) At 298 K, the standard enthalpies of formation for ethene C2H4 (8) and...
ANS is B 10. Ethene (ethylene, C2H4) can dimerize to produce cyclobutane (C4H8) in the presence of ultraviolet light: hvhH НН The average bond energies of C-H, C-C, and C C are 414 kj/mol, 347 k]/mol and 611 k]/mol, respectively. For this reaction, C. ΔΗΡ < 0 and AS° > 0
For the reaction: H2(g)+C2H4(g)-->C2H6(g) Bond & Bond Enthalpy H-H 436.4 kJ/mole C-H 414 kJ/mol C-C 347 kJ/mol C=C 620 kJ/mol Substance & delta Hf H2 0 C2H4 52.3 C2H6 -84.7 (a) estimate the enthalpy of reaction, using the bond enthalpy values from the table in kJ/mol (b) Calculate the enthalpy of reaction, using standard enthalpies of formation
for the following rxn Use the standard enthalpies of formation to calculate AH° reaction. C2H4(g) + H2(g) + C2H6(g) ΔΗ° Substance (kJ/mol) C₂H4 52.4 C2H6 -84.68 0 -32.3 kJ -4.3 x 103 kJ 32.3 kJ 0 -137.1 kJ
Consider the following values of standard enthalpies and free energies of formation at 298 K: Chemical Species C2H2(g) C2H6(g) AH (kJ mol-') +228 -84 AGI° (kJ moll) +211 -32 Determine whether the reaction: C2H2(g) + 2 H2(g) → C2H6(g) is: • spontaneous and exothermic • spontaneous but endothermic • non-spontaneous and exothermic • non-spontaneous but endothermic Show your working
Hydrocarbons, compounds containing only carbon and hydrogen, are important in fuels. The heat of combustion of cyclohexane, C6H12, is 936.8 kcal/mol. Write a balanced equation for the complete combustion of cyclohexane. + + How much energy is released during the complete combustion of 309 grams of cyclohexane ? kcal b.Combustion reactions are exothermic. The heat of reaction for the combustion of octane, C8H18, is 1.308×103 kcal/mol. What is the heat of combustion for octane in kcal/gram? kcal/gram...
Using the standard enthalpy of formation data, show how the standard enthalpy of formation of HF(g) can be used to determine the bond energy. (Enter unrounded values.) (a) bond energy calculated from standard enthalpy of formation kJ/mol (b) average bond enthalpy from the bond enthalpy table k]/mol Average Bond Enthalpies bondAH bond (kJ/mol) bond AHbond (kJ/mol) bond AH bond (kJ/mol) bond AH bond (kJ/mol) O-H 0-0 467 146 495 185 203 156 364 522 335 544 413 347 614 839...
Calculate the standard Gibbs energy change for the following generic reaction at 298 K, using the standard enthalpies of formation and standard entropies from the table below A+B-C AHI KJ SI JKT Substance mor1 mor1 148.0 299.0 0 76.2 -269.9 105.3 Select one: O a. 8.001e4 kJ/mol O b.-337.5 kJ/mol O C.-265.1 kJ/mol O d. 382.9 kJ/mol o e.-3.460e4 kJ/mol
c) The standard enthalpies of formation and molar entropies of phosgene, carbon monoxide, and chlorine are COCl2(g): ΔfH° = -220.08 kJ mol-1; S° = 283.8 J mol-1 K-1 CO(g): ΔfH° = -110.53 kJ mol-1; S° = 197.66 J mol-1 K-1 Cl2(g): ΔfH° = 0 kJ mol-1; S° = 223.08 J mol-1 K-1 i) Determine the reaction Gibbs energy for the decomposition of phosgene at 298 K. Is this reaction spontaneous at this temperature? [25 marks] ii) At what temperature does...
Use standard enthalpies of formation (in Appendix G in text) to calculate ∆H°rxn for each reaction. ∑ m∆H°f (products) - ∑n∆H°f (reactants), where m and n are coefficients. C2H4(g) + H2(g) ----- > C2H6(g) CO (g) + H2O (g) ----- > H2(g) + CO2(g) 3NO2(g) + H2O (l) ----- > 2HNO3(aq) + NO (g) 2SO2(g) + O2(g) -----------> 2SO3(g) 2C4H10 (g) + 13O2 (g) -----------> 8CO2 (g) + 10H2O (g) Substance --- ΔH° (kJ mol–) --- ΔG° (kJ mol–1) --- S°298 (J K–1 mol–1) C2H4 52.4 86.4 219.3 H2 0 0 130.7 C2H6 -84.0 -32.0 229.2 CO -110.52 -137.15 197.7 H2O -285.83 -237.1 70.0 CO2 -393.51 -394.36 213.8 NO2 33.2 51.30 240.1 NO 90.25 87.6 210.8 SO2 -296.83 -300.1 248.2 O2 0 0 205.2 SO3 -395.72 -371.06 256.76
The standard heat of formation for FeCl3(s) is -400 kJ/mol at 298 K. Write the formation equation for FeCl3(8) that goes with this value of ΔΗ. Use the pull-down boxes to specify states. Write fractions with a slash, such as 1/2 for one half. If a box is not needed leave it blank.