Calculate the standard enthalpy change of reaction (ΔH°) for the following reaction using the reaction enthalpies and the standard enthalpies of formation (ΔHf°) of the reactants and products:

2SO2(g) + O2(g) -> 2SO3(g)

Given: ΔHf° (SO2) = -296.8 kJ/mol ΔHf° (O2) = 0 kJ/mol ΔHf° (SO3) = -395.6 kJ/mol

Note: All enthalpy changes are given per mole of substance.

3. You are given the following standard enthalpies of formation at 25°C HF (aq OH (aq) F (aq) H20 (1) -320.1 kJ/mol -229.6 kJ/mol -329.1 kJ/mol -285.8 kJ/mol a. Calculate the standard enthalpy of neutralization of HF (aq) HF (aq) + OH. (aq) → F (aq) + H2O (1) b. Using the value of -56.2 kJ/mol as the standard enthalpy change for the reaction H+ (aq) + OH. (aq) H2O ( 1 ) → calculate the standard enthalpy change for the reaction HF (aq) H' (aq) F (aq) -一→ 4. You are given the following information. =-4.8 kJ dH ΔH = 29.1 kJ N:04 (g) N2 (g) + 202 (g) 2NO2 (g) → N204 (g) → determine the enthalpy change ( ) for the reaction: N2(g) + 202 (g) 2 NO2(g)

A scientist measures the standard enthalpy change for the following reaction to be -2922.0 kJ: 2C_2 H_6 (g) + 7 O_2 (g) 4CO_2 (g) + 6 H_2 O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H_2 O(g) is kJ/mol.