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

Calculate ΔHrxn for the following reaction using Hess's Law: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g). Given the following reactions and their ΔH values: 1) 2Fe(s) + 3/2O2(g) → Fe2O3(s), ΔH = -824.2 kJ; 2) CO(g) + 1/2O2(g) → CO2(g), ΔH = -282.7 kJ.

Calculate ΔH_rxn for the reaction: N2O (g) + NO2 (g) → 3 NO (g) using the following reactions and given ΔH values: 1) 2 NO (g) + O2 (g) → 2 NO2 (g), ΔH = -113.1 kJ; 2) N2 (g) + O2 (g) → 2 NO (g), ΔH = +182.6 kJ; 3) 2 N2O (g) → 2 N2 (g) + O2 (g), ΔH = -163.2 kJ.

Calculate ΔH⁰ for the process 1/2 N2(g) + 1/2 O2(g) → NO(g) using Hess's Law and the following reactions: 1. N2(g) + 3 H2(g) → 2 NH3(g) ΔH⁰ = -91.8 kJ 2. 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) ΔH⁰ = -906.2 kJ 3. H2(g) + 1/2 O2(g) → H2O(g) ΔH⁰ = -241.8 kJ

Using Hess's Law, calculate the ΔH for the reaction: N2(g) + 2O2(g) ---> 2NO2(g) using the following data:1. 2 NH3(g) + 4 H2O(l) ---> 2 NO2(g) + 7 H2(g) ΔH = −142.4 kJ2. N2(g) + 3H2(g) ---> 2NH3(g) ΔH = −115 kJ3. H2O(l) ---> H2(g) + 1/2 O2(g) ΔH = −43.7 kJ

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 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