3. Calculate the heat of reaction, A Hrxn, for the decomposition of barium carbonate into barium oxide and carbon dioxide. Standard enthalpy of formation data are provided below. AH° {(BaCO3) = -1216.3 kJ/mol AH° f(BaO) = -553.5 kJ/mol AH° ¡(CO2) = -393.5 kJ/mol %3D

The following is the balanced equation for the reaction of gaseous ammonia with oxygen gas.                       4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g)   Using the ΔHf° values shown below, calculate the ΔHrxn° for the overall reaction.        ΔHf°(NO (g)) = 91.3 kJ/mol      ΔHf°(NH3 (g)) = −45.9 kJ/mol      ΔHf°(H2O (l)) = −241.8 kJ/mol A) −294.8 kJ/mol B) −731.5 kJ/mol C) −902.0 kJ/mol D) −468.2 kJ/mol

Consider the reaction.   2Fe2O3⟶4Fe+3O2        Δ?∘rxn=+824.2 kJ   The decomposition of 74.0 g of Fe2O3 results in A.) the release of 382 kJ of heat. B.) the absorption of 191 kJ of heat. C.) the release of 191 kJ of heat. D.) the absorption of 30500 kJ of heat. E.) the release of 30500 kJ of heat. F.) the absorption of 382 kJ of heat.

2. Please calculate the standard enthalpy of reaction (AHrxn, in kJ/mol) for the preparation of nitrous acid, HNO2, using the thermodynamic data given below. Preparation of nitrous acid: HCl(g) + NaNO2(s) → HNO2(1) + NaCl(s) 2NaCl(s) + H₂O(l) → 2HCl(g) + Na₂O(s) NO(g) + NO₂(g) + Na2O(s) → 2NaNO2 (s) NO(g) + NO₂(g) → N₂O(g) + O₂(g) 2HNO2(1)→ N₂O(g) + O2(g) + H₂O(g) H₂O(1)→ H₂O(g) ΔΗ = 507.31 kJ/mol AH = -427.14 kJ/mol AH = - 42.68 kJ/mol 34.35 kJ/mol ΔΗ ΔΗ = 44.012 kJ/mol =

Consider the reaction. 2 Fe₂0₂4Fe +30₂ AHin = +824.2 kJ The formation of 62.0 g of Fe results in the release of 229 kJ of heat. the absorption of 229 kJ of heat. O the release of 12800 kJ of heat. the release of 915 kJ of heat. the absorption of 12800 kJ of heat. the absorption of 915 kJ of heat.

Calculate ΔH° for the reaction shown below using standard enthalpy of formation values. KCl (s)   →   K+1 (aq)   +   Cl-1 (aq) Be sure to include a unit with your answer.