Consider the combination reaction: 2Mg(s) + O2(g) → 2MgO(s) with ΔH = -1204 kJ. What is the enthalpy change for the decomposition of 1 mole of MgO(s) into Mg(s) and O2(g)?

Calculate the enthalpy change for the reaction: NO(g) + O(g) -> NO2(g), given the following standard enthalpies of formation: ΔHf°[NO(g)] = 90.25 kJ/mol, ΔHf°[O(g)] = 249.17 kJ/mol, ΔHf°[NO2(g)] = 33.18 kJ/mol.

Calculate the standard enthalpy change for the following reaction at 25°C using the standard enthalpies of formation: C3H8 (g) + 5O2 (g) -> 3CO2 (g) + 4H2O (g). Given: ΔHf° [C3H8 (g)] = -104.7 kJ/mol, ΔHf° [CO2 (g)] = -393.5 kJ/mol, ΔHf° [H2O (g)] = -241.8 kJ/mol.

Choose the reaction that illustrates the standard enthalpy of formation (ΔHf°) for Ca(NO2)2.

Which of the following reactions represents the standard enthalpy of formation (ΔHₒƒ) for CsHSO4(s)?

Which of the following statements correctly describes the calculation of the enthalpy change (ΔH_rxn) for a chemical reaction using bond enthalpies?

What is the standard enthalpy of formation of the isomer C8H18 if the enthalpy change for its complete combustion is -5470 kJ/mol?

For which of the following reactions is the enthalpy change for the reaction equal to the standard enthalpy of formation (ΔHf°) of the product?

The enthalpy change for the following reaction is -483.6 kJ: 2 H2 (g) + O2 (g) --> 2 H2O (g). Therefore, the enthalpy change for the following reaction is ________ kJ: 6 H2O (g) --> 6 H2 (g) + 3 O2 (g).