Calculate the∆Hrxnfor the following thermochemical equation:

When given the following:

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

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.

Find ΔH_rxn for the following reaction:

N₂ + 2 O₂ → 2 NO₂
Based on the following data.
2 NO → N₂ + O₂    ΔH = −180 kJ
2 NO + O₂ → 2 NO₂    ΔH = −112 kJ

Calculate the enthalpy change for the reactionC(s) + 2 H2(g) → CH4(g) ΔH = ?Given the enthalpy values for the following reactionsCH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ΔH = −890.4 kJC(s) + O2(g) → CO2(g) ΔH = −393.5 kJH2(g) + 1/2 O2(g) → H2O (g) ΔH = −285.8 kJ(a) −1569.7 kJ(b) +211.1 kJ(c) −1855.5 kJ(d) −74.7 kJ