Using the equations below, determine the molar enthalpy change (ΔH°) for the combustion of octane (C₈H₁₈) in kJ/mol. 1. 2 C₈H₁₈ (l) + 15 O₂ (g) → 12 CO₂ (g) + 6 H₂O (g) ΔH° = -6271 kJ/mol2. 2 H₂ (g) + O₂ (g) → 2 H₂O (g) ΔH° = -483.6 kJ/mol3. C (s) + O₂ (g) → CO₂ (g) ΔH° = -393.5 kJ/mol

Determine the enthalpy of reaction for 2CH₄(g) → C₂H₂(g) + 2H₂(g) using the given equations and Hess's Law.

Using Hess's Law, calculate the enthalpy change for the reaction: 2 Cl(g) + O2(g) → 2 ClO2(g), given that a chlorine-oxygen bond in ClO2(g) has an enthalpy of 243 kJ/mol, an oxygen-oxygen bond has an enthalpy of 498 kJ/mol, and the standard enthalpy of formation of ClO2(g) is ΔH°f = 102.5 kJ/mol.

Given the following reactions:2S (s) + 3O2 (g) → 2SO3 (g) ΔH = -790 kJS (s) + O2 (g) → SO2 (g) ΔH = -297 kJWhat is the enthalpy change (ΔH) for the reaction in which sulfur dioxide is oxidized to sulfur trioxide: 2SO2 (g) + O2 (g) → 2SO3 (g)?

Using Hess's Law, calculate the standard Gibbs free energy change (ΔG°_rxn) for the reaction: ClO(g) + O3(g) → Cl(g) + 2 O2(g), given the following reactions and their ΔG°_rxn values: 1) 2 O3(g) → 3 O2(g), ΔG°_rxn = +489.6 kJ; 2) Cl(g) + O3(g) → ClO(g) + O2(g), ΔG°_rxn = -101.3 kJ.

Using Hess's Law, calculate the enthalpy change for the formation of water (H₂(g) + 1/2 O₂(g) → H₂O(l)) given the following reactions: Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g) with ΔH_rxn = -385 kJ/mol and MgO(s) + 2HCl(aq) → MgCl₂(aq) + H₂O(l) with ΔH_rxn = -80 kJ/mol.