Consider the reaction 2 S(g) + 3 O2(g) → 2 SO3(g). Using the standard enthalpies of formation listed in Appendix G of your text and the bond energy of 498.4 kJ/mol in molecular oxygen, calculate the average sulfur-oxygen bond energy, in units of kJ/mol, in sulfur trioxide gas. The answer is not 473!

Based on the bond energies for the reaction below, what is the enthalpy of the reaction? HC≡CH (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (g)

1. Draw Lewis structures for ozone and for dioxygen. Using the data given below, qualitatively compare the bond enthalpies, bond orders, and bond lengths of these two compounds. O₂ (g) 20 (g) AH" = +498 kJ O(g) + O₂(g) →O, (g) AH-105 kJ

A certain element X forms two compounds with hydrogen, XH3 and X2H4 (H2X–XH2). The total bond enthalpies of XH3(g) and X2H4(g) are 846 kJ/mol and 1341 kJ/mol, respectively. What is the average bond enthalpy of the X–X bond?

Cyanamide is a compound containing two hydrogen atoms and some amount of C and N. There are a total of 5 atoms in the compound. The products of combustion were found to be CO2, NO2, and H2O. If the enthalpy of combustion for cyanamide is – 671.9 kJ/mol and the enthalpy of formation is 58.8 kJ/mol, what is the chemical formula for cyanamide? ( ΔfH (CO2) = - 393.51 kJ/mole; ΔfH (NO2) = + 33.10 kJ/mole; ΔfH (H2O) = - 241.826 kJ/mole)

Hydrazine is an inorganic compound with the chemical formula N₂H4. The reaction of hydrazine with chlorine trifluoride has been used in experimental rocket motors in the reaction below: 3N₂H4 (1) + 4CIF3 (g) → → 3N2 3N2 (g) (g) + 12HF Calculate enthalpy change for the reaction given the following: (1) 2CIF3 + 2NH3N₂ + 6HF + Cl₂ (2) N₂H4 + O₂ → N₂ + 2H₂O (3) 4NH3 + 302 → 2N₂ + 6H₂O (g) Search + 2Cl2 (g) AH = -1196 kJ AH°=-622 kJ AH° = - 1530 kJ Using ethanol as a fuel reduces greenhouse gas emissions by 40-50% when compared directly to ha enthalpies of

Use the data in Thermodynamic Properties and the bond energy in Bond Energies to determine the average C-C bond energy in benzene (C6H₁). 4.0✔ kJ/mol Calculate the average of a C-C single bond and a C=C double bond using the bond energies, which is the value expected from the Lewis structure. 4.0✔ kJ/mol The larger calculated value using thermodynamic properties is due to the fact that the pi system is delocalized, which makes the molecule more stable than predicted by simply averaging the C-C bonds.

Use the molar bond enthalpy data in the table to estimate the value of AHin for the equation CC14(g) + 2 F₂ (g) → CF₁ (g) + 2 Cl₂ (g) 2 The bonding in the molecules is shown. ΔΗ +=++· rxn = -CI F-F F-F -C-F CI-CI CI-CI Average molar bond enthalpies (Hbond) Bond Bond O-H C=N 0-0 N-H C-O N-N 0=0 N=N C=O N=N C-C F-F C=C Cl-Cl C=C Br-Br C-H H-H C-F H-F C-Cl H-Cl C-Br H-Br C-N H-S C=N S-S kJ.mol-¹ 464 142 351 502 730 347 615 811 414 439 331 276 293 615 kJ.mol-1 890 390 159 418 945 155 243 192 435 565 431 368 364 225 kJ.mol-¹

Use the bond energies provided for the question

Using average bond enthalpies, estimate the enthalpy change for the following reaction: 2CO(g) + O2(g) → 2CO₂(g) AHrxn Bond Bond Energy (kJ/mol) C=O 1072 0=0 498 C=O 732 kJ