The heat of combustion of ethyne, carbon, and hydrogen gas are -1300 kJ/mol, - 394 kJ/mol and -286 kJ/mol respectively. By manipulating the information given, calculate the enthalpy of formation of ethyne from the reaction between carbon and hydrogen gas.

6. Heat of Formation. Give the balanced chemical equation used to find the heat of formation of the following a) CH3COOH (1) b) Na2SO4(s)

Question 32 of 37 Use the following table of bond energies to calculate the molar enthalpy of combustion (in kJ/mol) of acetylene (C2H2) gas in oxygen, based on the following chemical equation: C2H2(g) + 2.502(g) → 2CO:(g) + H2O(g) Single H Bond H 2057 kJ/mol 432 C 411 346 386 305 167 459 358 201 142 1 2 3 C=C 602 C=O 799 C=C 835 C=O 1072 Multiple Bonds 4 6. C=N 615 O=O 494 C=N 887 N=N 942 **All values in kJ/mol** 7 8 9. +/- CO LO

What is the heat of combustion of ethane, C₂H, in kilojoules per mole of ethane? Enthalpy of formation values can be found in this list of thermodynamic properties. AH = kJ/mol ethane

a) Write a balanced reaction for the combustion of methane.b) Calculate the heat of combustion of methane, in kJ/mol.c) Calculate the energy content of methane. The energy content of a fuel is the energy released per gram of fuel (whereas the heat of combustion is the energy per mole of fuel).d) How many grams of CO2 will be released for every gram of methane that you burn?e) How many grams of CO2 will be released for every kJ of energy produced by the combustion of methane?