Question 7. Use the bond energies provided to estimate ΔH°rxn for the reaction below. CH3OH(l) + 2 O2(g) → CO2(g) + 2 H2O(g) ΔH°rxn = ? Bond Bond Energy (kJ/mol) C-H 410 C-O 359 C=O 799 O=O 498 O-H 454

Nitesh

thway | Algebra. Pt Periodic Table - Pta... Scientific Calculator Gravitational Force... Conservation of Mo... Part 1-Combustion of Methane Equation for Enthalpy AH = Hbonds broken- Hsonds formed The following table is a list of selected bond energies. The bonds present in this table are common bonds for combustion reactions Selected Bond Energies Bond Energy (kI/mole) Bond Bond Energy Bond (kl/mole) H-H 436 C=0 799 O-0 495 C-C 348 O-H 463 C=C 614 C-H 413 C-C (aromatic) 519 C-O 358 N=0 623 Use the following balanced equation and chart to complete the bond energy calculations for the fuel, methane CH+202-CO2+2 H20 Compound Total Bond Energy Oxygen, O2 495 kJ/mol Carbon Dioxide, CO, 1598 kl/mol Water, H,O 926 kJ/mol

1. What is the enthalpy of reaction per mole of HCl (g) in the following reaction.( Don't have to explain why) 4HCl (g) + O2 (g) → 2Cl2 (g) + 2H2O + 114.4 kJ a) -457.6 kJ / mol b) -114.4 kJ / mol c) -28.6 kJ / mol d) +114.4 kJ / mol 2. The standard enthalpy of formation of a compound represents: a) The thermal energy released by the decomposition of one mole of this compound. b) The change in enthalpy when a mole of this compound is formed from its elements under standard conditions. c) The change in enthalpy when one mole of an element turns into a compound. d)The thermal energy released by the complete combustion of one mole of this compound. e) The enthalpy change of the phase transition of one mole of this compound.