Using average bond energies and the standard enthalpy of formation of C(g) (718.4 kJ/mol), estimate the standard enthalpy of formation of gaseous benzene, C6H6(g). Which of the following values is closest to the correct estimate?

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).

Given the reaction Pb (s) + CO2 (g) → PbO (s) + CO (g) with ΔH° = +131.4 kJ, and the standard enthalpies of formation ΔHf° of CO2(g) = -393.5 kJ/mol and CO(g) = -110.5 kJ/mol, what is the standard enthalpy of formation for PbO(s)?

The enthalpy for the formation of 1 mole of NH₃(aq) is -80.29 kJ/mol. What is the enthalpy for the formation of 3 moles of NH₃(aq)?

Given the heat of formation of TiI3(s) is -328 kJ/mol and the heat of reaction for 2Ti(s) + 3I2(g) → 2TiI3(s) is -839 kJ, what is the heat of sublimation of I2(s) at 25°C?

Use standard enthalpies of formation to calculate ΔH°_rxn for the following reaction: C(s) + H₂O(g) → CO(g) + H₂(g). Given the standard enthalpies of formation: ΔH°_f [C(s)] = 0 kJ/mol, ΔH°_f [H₂O(g)] = -241.8 kJ/mol, ΔH°_f [CO(g)] = -110.5 kJ/mol, ΔH°_f [H₂(g)] = 0 kJ/mol.

Use standard enthalpies of formation to calculate ΔHºrxn for the following reaction: 2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g). Which of the following is the correct value for ΔHºrxn?

Use standard enthalpies of formation to calculate ΔH°rxn for the following reaction: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g). Given the following standard enthalpies of formation: CH4(g) = -74.8 kJ/mol, CO2(g) = -393.5 kJ/mol, H2O(g) = -241.8 kJ/mol, O2(g) = 0 kJ/mol.

Using the standard enthalpies of formation, calculate ΔH°rxn for the reaction: CaO(s) + CO2(g) → CaCO3(s). Given: ΔH°f [CaO(s)] = -635.1 kJ/mol, ΔH°f [CO2(g)] = -393.5 kJ/mol, ΔH°f [CaCO3(s)] = -1206.9 kJ/mol.