23. Given the following reactions, calculate the enthalpy of the reaction of N2 and O2 to produce nitric oxide. (Ref: pgs. 181-182) N2 (g) + 2 O2 (g) 2NO2 (g) = 66.4 kJ → ΔH 2NO (g) + O2 (g) 2NO2 (g) = -114.2 kJ → ΔH N2 (g) + O2 (g) 2NO (g) = ??? → ΔH 24. Consider the following two reactions: A 2B = 456.7 kJ/mol → ΔH°rxn A C = -22.1kJ/mol → ΔH°rxn Determine the enthalpy change for the process: 2B C (Ref: pg. 187, sample 5.12) → 25. Given the data in the table below, calculate for the reaction: (Ref: pg. 187, sample 5.11) ΔH°rxn Ca(OH)2 + 2 H3AsO4 Ca(H2AsO4)2 + 2 H2O →
23. Given the following reactions, calculate the enthalpy of the reaction of N2 and O2 to produce nitric oxide. (Ref: pgs. 181-182) N2 (g) + 2 O2 (g) → 2NO2 (g) ΔH = 66.4 kJ 2NO (g) + O2 (g) → 2NO2 (g) ΔH = -114.2 kJ N2 (g) + O2 (g) → 2NO (g) ΔH = ??? 24. Consider the following two reactions: A → 2B ΔH°rxn = 456.7 kJ/mol A → C ΔH°rxn = -22.1kJ/mol Determine the enthalpy change for the process: 2B → C (Ref: pg. 187, sample 5.12) 25. Given the data in the table below, calculate ΔH°rxn for the reaction: (Ref: pg. 187, sample 5.11) Ca(OH)2 + 2 H3AsO4 → Ca(H2AsO4)2 + 2 H2O
ap_thermochemistry_wkst_1.docx