Chap_6_HW_solutions

Chap_6_HW_solutions - Chapter 6 homework solutions

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Chapter 6 Homework Solutions 28. As a system increases in volume, it absorbs 52.5 J of energy in the form of heat from the surroundings. The piston is working against a pressure of 0.500 atm. The final volume of the system is 58.0 L. What was the initial volume of the system if the internal energy of the system decreased by 102.5 J? 30. One mole of H 2 O (g) at 1.00 atm and 100. o C occupies a volume of 30.6 L. When one mole of H 2 O (g) is condensed to one mole of H 2 O (l) at 1.00 atm and 100. o C, 40.66 kJ of heat is released. If the density of H 2 O (l) at this temperature and pressure is 0.996 g/cm 3 , calculate E for the condensation of one mole of water at 1.00 atm and 100. o C.
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34. Are the following processes exothermic or endothermic? a. the combustion of gasoline in a car engine b. water condensing on a cold pipe c. CO 2 (s) CO 2 (g) d. F 2 (g) 2 F (g) 36. Consider the following reaction: 2 H 2 (g) + O 2 (g) 2 H 2 O (l) H = -572 kJ a. How much heat is evolved for the production of 1.00 mol of H 2 O (l) ? b. How much heat is evolved when 4.03 g of hydrogen is reacted with excess oxygen? c. How much heat is evolved when 186 g of oxygen is reacted with excess hydrogen? d. The total volume of hydrogen gas needed to fill the Hindenburg was 2.0 x 10 8 L at 1.0 atm and 25 o C. How much heat was evolved when the Hindenburg exploded, assuming all of the hydrogen reacted?
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44. It takes 585 J of energy to raise the temperature of 125.6 g of mercury from 20.0
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Chap_6_HW_solutions - Chapter 6 homework solutions

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