Given the following data:    2C2H6 (g) + 7O2 (g) ------> 4CO2 (g) + 6H2 (g)             ΔH= -3120kJ C (s) + O2 (g) -----> CO2 (g)                                          ΔH= -394kJ 2H2 (g) + O2 (g) ----->  2H2O (l)                                     ΔH= -572kJ Use Hess’s law to calculate ΔH for the reaction: 2C(s) + 3H2 (g) -----> C2H6 (g)   ΔH= Answer.................. kJ

2. Consider the following thermochemical equations: C(graphite) + O2 (g) → co2 (g) AH°rn = -393.5 kJ H2 (g) + % 02 (g) → H;0 (/) AHO = -285.8 kJ 2 C:Hs (g) + 702 (g) → 4 CO2 (g) + 6 H20 (1) AH°rn = -3119.6 kJ a. Derive the thermochemical equation describing the combustion of two moles of C(graphite). b. Derive the thermochemical equation describing the combustion of three moles of H2 (g). c. Derive the thermochemical equation describing the synthesis of one mole of C,Hg (9) from carbon dioxide and water. d. Use Hess's Law and the three thermochemical equations you derived in parts a-c to determine the AH°ran for the following reaction: 2C (graphite) + 3 H2 (g) → C;Hs (g)

To study the possible amount of energy generated by a person, the person can be roughly viewed as a constant pressure calorimeter using table sugar (sucrose, C12H22O11) as the energy generator. The reaction of table sugar in a calorimeter is given by: C12H22O11(s) + 12O2(g) ----------> 12CO2(g) + 11H2O(g)   a. What is the heat released by consuming one mole of sugar (C12H22O11) in this way? b. Calculate the enthalpy of combustion per mole of sugar utilization. c. Does the result of your calculation make sense?

Given the following thermochemical equations: C2H29) + 5 02(9) 2C02(g) + H201) AH° = -1229.5 kJ AH° = -393.5 kJ C(6) + 02(g) → C02(g) 1 H2(9) +5 02(9) → H20) AH° = -285.5 kJ 2 Calculate the enthalpy (in kJ) for this reaction: 206) + H2(g) → C,H2(9)