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

THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (g) + 3J2X (1) AH = -1,070 kJ 4QJ3 (g) + 3X2 (g) → 202 (g) + 6J2X (1) AH = -1,580.2 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + % X2 (g) –→ Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.)

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?

THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (9) + 3J2X (1) AH = -1,017.3 kJ 4QJ3 (g) + 3X2 (g) → 202 (9) + 6J2X (1) AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + % X2 (g) –→ Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.)

Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give carbon dioxide and water. 2C8H18(l)+25O2(g)⟶16CO2(g)+H2O(l)2C8H18(l)+25O2(g)⟶16CO2(g)+H2O(l)           ΔH=−10,922kJΔH=−10,922kJ Calculate the mass, in g, of C8H18C8H18 that reacts if 6112.23 kJ of heat is released in the process.

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)

A sample of steam with a mass of 0.506 g at a temperature of 100 ∘C condenses into an insulated container holding 4.20 g of water at 3.0 ∘C . For water, ΔH∘vap=40.7kJ/mol and Cwater=4.18J/(g⋅∘C) .

Determine the standard nolar enthalpy change ∆H°rxn (in kilojoules per mole) for the following reactio given below.  2Pb(NO3)2 (s) --> 2PbO(s) + 4NO2(g) + O2(g)

Use the thermochemical equations shown below to determine the enthalpy for the reaction: C3H8(g) + 502(g) +3CO 2 + 4H2O(1) CO2 C(graphite) + 02 HE = 221.6KJ H2(g) + 1/2O2(g) H2O(1) HE= -160.3KJ 3 C(graphite) + 4 H2(g) C3H8(g) HE= -58.5KJ