Calculate ΔH° for the combustion of methane. CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g) Given the enthalpies of formation below. CH4 (g): -50.8 kJ/molO2 (g); 0 kJ/molCO2 (g); -394.4 kJ/molH2O (g); -228.57 kJ/mol

Substance AH (kJ/mol) MgCl2(aq) -785.1 kJ/mol HCl(aq) -167.2 kJ/mol Given the enthalpy of formation data in the table, what is the enthalpy of reaction for the reaction you performed in this lab? To calculate the enthalpy of reaction, use the following formula. AHrxn =ΣAH(products) - ΣAH; (reactants) Note that you will need the balanced chemical equation for the reaction performed in the lab. Also, note that AH; for the standard state elements is 0 kJ/mol. AHrxn = Is the calculated result simliar to the experimentally determined result? yes no kJ/mol

A scientist measures the standard enthalpy change for the following reaction to be -876.7 kJ :2NH3(g) + 3 N2O(g)4N2(g) + 3 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of NH3(g) is kJ/mol.

Use the standard molar enthalpies of formation and calculate the change in enthalpy for the reaction :                                            2CH3OH (l) + 3O2 (g) --> 2CO2 (g) + 4H2O (l) Given: CH3OH(l): -238.4 kJ/mol O2(g): 0 kJ/mol CO2(g): -393.5 kJ/mol H2O(l): -285.83 kJ/mol