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CHAPTER 6 SG

# CHAPTER 6 SG - Calculate ∆ H rxn for the following...

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CHAPTER 6: STUDY GUIDE Define thermochemistry and energy. State the law of conservation of energy. What are potential and kinetic energy? Define heat and work. What is a state function? What are the system and surroundings? How are exothermic reactions different from endothermic reactions? How do you calculate internal energy? What is enthalpy and how is it calculated? What mass of natural gas (CH 4 ) must you burn to emit 267 kJ of heat? CH 4 (g) + 2 O 2(g) → CO 2 (g) + 2 H 2 O (l) H o rxn = -802.3 kJ Define calorimetry, heat capacity and molar heat capacity. What are the steps involved in solving calorimetry problems? A 25.5 g aluminum block is warmed to 65.4 o C and plunged into an insulated beaker containing 55.2 g water initially at 22.2 o C. The aluminum and the water are allowed to come to thermal equilibrium. Assuming that no heat is lost, what is the final temperature of the water? What is Hess's law? What are two important characteristics of enthalpy changes?

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Unformatted text preview: Calculate ∆ H rxn for the following reaction: CH 4 (g) + 4 Cl 2 (g) → CCl 4 (g) + 4 HCl (g) Use the following reactions and given ∆ H's. C (s) + 2 H 2 (g) → CH 4 (g) ∆ H = -74.6 kJ C (s) + 2 Cl 2 (g) → CCl 4 (g) ∆ H = -95.7 kJ H 2 (g) + Cl 2 (g) → 2 HCl (g) ∆ H = -92.3 kJ Define standard enthalpy of formation. What are standard states for compounds and elements and at what temperature and pressure are they determined at? How do you determine the standard enthalpy of a reaction? Hydrazine (N 2 H 4 ) is a fuel used by some spacecraft. It is normally oxidized by N 2 O 4 according to the following equation: N 2 H 4 (l) + N 2 O 4 (g) → 2 N 2 O (g) + 2 H 2 O (g) Calculate ∆ H o rxn for this reaction using standard enthalpies of formation. ∆ H o f N 2 H 4 = 50.6 kJ/mol ∆ H o f N 2 O 4 = 11.1 kJ/mol ∆ H o f N 2 O = 81.6 kJ/mol ∆ H o f H 2 O = -241.8 kJ/mol...
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CHAPTER 6 SG - Calculate ∆ H rxn for the following...

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