Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 5, Problem 61PS
The standard enthalpy of formation of solid barium oxide, BaO, is –553.5 kJ/mol, and the standard enthalpy of formation of barium peroxide, BaO2, is –634.3 kJ/mol.
(a) Calculate the standard enthalpy change for the following reaction. Is the reaction exothermic or endothermic?
2 BaO2(s) → 2 BaO(s) + O2(g)
(b) Draw an energy level diagram that shows the relationship between the enthalpy change of the decomposition of BaO2, to BaO and O2, and the enthalpies of formation of BaO2(s) and BaO2(s).
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Chapter 5 Solutions
Chemistry & Chemical Reactivity
Ch. 5.1 - 1. Which of the following processes is...Ch. 5.1 - 2. Your skin cools as perspiration evaporates. Is...Ch. 5.2 - You did an experiment in which you found that 59.8...Ch. 5.2 - A 15.5-g piece of chromium, heated to 100.0 C, is...Ch. 5.2 - Prob. 1RCCh. 5.2 - Prob. 2RCCh. 5.3 - Calculate the amount of energy necessary to raise...Ch. 5.3 - To make a glass of iced tea, you pour 250 mL of...Ch. 5.3 - 1. Which of the following processes requires the...Ch. 5.3 - Ice (5.0 g) at 0 C is added to 25 g of liquid...
Ch. 5.4 - Nitrogen gas (2.75 L) is confined in a cylinder...Ch. 5.4 - Which of the following processes will lead to a...Ch. 5.4 - 2. In which of the following reactions is there a...Ch. 5.5 - The combustion of ethane, C2H6, has an enthalpy...Ch. 5.5 - 1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s),...Ch. 5.5 - 2. For the reaction 2 CO(g) + O2(g) → 2 CO2(g)....Ch. 5.6 - Assume 200. mL of 0.400 M HCl is mixed with 200....Ch. 5.6 - A 1.00-g sample of ordinary table sugar (sucrose,...Ch. 5.6 - A student used a coffee-cup calorimeter to...Ch. 5.6 - If, in the experiment described in the previous...Ch. 5.7 - Use Hesss law to calculate the enthalpy change for...Ch. 5.7 - Calculate the standard enthalpy of combustion for...Ch. 5.7 - Prob. 1RCCh. 5.7 - The standard enthalpies of formation of KNO3(s)...Ch. 5.7 - Prob. 2QCh. 5.7 - The decomposition of nitroglycerin (C3H5N3O9)...Ch. 5.7 - Prob. 2RCCh. 5 - Define the terms system and surroundings. What...Ch. 5 - What determines the directionality of energy...Ch. 5 - Identify whether the following processes are...Ch. 5 - Identify whether the following processes are...Ch. 5 - The molar heat capacity of mercury is 28.1 J/mol ...Ch. 5 - The specific heat capacity of benzene (C6H6) is...Ch. 5 - The specific heat capacity of copper metal is...Ch. 5 - How much energy as heat is required to raise the...Ch. 5 - The initial temperature of a 344-g sample of iron...Ch. 5 - After absorbing 1.850 kJ of energy as heat, the...Ch. 5 - A 45.5-g sample of copper at 99.8 C is dropped...Ch. 5 - One beaker contains 156 g of water at 22 C, and a...Ch. 5 - A 182-g sample of gold at some temperature was...Ch. 5 - When 108 g of water at a temperature of 22.5 C is...Ch. 5 - A 13.8-g piece of zinc is heated to 98.8 C in...Ch. 5 - A 237-g piece of molybdenum, initially at 100.0 C,...Ch. 5 - How much energy is evolved as heat when 1.0 L of...Ch. 5 - The energy required to melt 1.00 g of ice at 0 C...Ch. 5 - How much energy is required to vaporize 125 g of...Ch. 5 - Chloromethane, CH3CI, arises from microbial...Ch. 5 - The freezing point of mercury is 38.8 C. 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CO2(s), forms...Ch. 5 - In the reaction of two moles of gaseous hydrogen...
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