9th Edition

ISBN: 9781133949640

Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher: Cengage Learning

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Textbook Question

Chapter 5.4, Problem 2RC

In which of the following reactions is there a significant transfer of energy as work from the system to the surroundings? This occurs if there is a change in the number of moles of gases.

(a) C(s) + O₂(g) → CO₂(g)
(b) CH₄(g) + 2 O₂(g) → CO₂g) + 2 H₂O(g)
(c) 2 C(s) + O₂(g) → 2 CO(g)
(d) 2 Mg(s) + O₂(g) → 2 MgO(s)

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Chapter 5.4, Problem 1RC

Chapter 5.5, Problem 1CYU

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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. 1RC Ch. 5.2 - Prob. 2RC Ch. 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. 1RC Ch. 5.7 - The standard enthalpies of formation of KNO3(s)...Ch. 5.7 - Prob. 2Q Ch. 5.7 - The decomposition of nitroglycerin (C3H5N3O9)...Ch. 5.7 - Prob. 2RC Ch. 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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CH3CO2H, is made industrially by the...Ch. 5 - You mix 125 mL of 0.250 M CsOH with 50.0 mL of...Ch. 5 - You mix 125 mL of 0.250 M CsOH with 50.0 mL of...Ch. 5 - A piece of titanium metal with a mass of 20.8 g is...Ch. 5 - A piece of chromium metal with a mass of 24.26 g...Ch. 5 - Adding 5.44 g of NH4NO3(s) to 150.0 g of water in...Ch. 5 - You should use care when dissolving H2SO4 in water...Ch. 5 - Sulfur (2.56 g) was burned in a constant-volume...Ch. 5 - Suppose you burned 0.300 g of C(s) in an excess of...Ch. 5 - Suppose you burned 1.500 g of benzoic acid,...Ch. 5 - A 0.692-g sample of glucose, C6H12O6, was burned...Ch. 5 - An ice calorimeter can be used to determine the...Ch. 5 - A 9.36-g piece of platinum was heated to 98.6 C in...Ch. 5 - The enthalpy changes for the following reactions...Ch. 5 - The enthalpy changes of the following reactions...Ch. 5 - Enthalpy changes for the following reactions can...Ch. 5 - You wish to know the enthalpy change for the...Ch. 5 - Write a balanced chemical equation for the...Ch. 5 - Write a balanced chemical equation for the...Ch. 5 - (a) Write a balanced chemical equation for the...Ch. 5 - (a) Write a balanced chemical equation for the...Ch. 5 - Use standard enthalpies of formation in Appendix L...Ch. 5 - Use standard enthalpies of formation in Appendix L...Ch. 5 - The first step in the production of nitric acid...Ch. 5 - The Romans used calcium oxide, CaO, to produce a...Ch. 5 - The standard enthalpy of formation of solid barium...Ch. 5 - An important step in the production of sulfuric...Ch. 5 - The enthalpy change for the oxidation of...Ch. 5 - The enthalpy change for the oxidation of styrene....Ch. 5 - Prob. 65GQ Ch. 5 - Prob. 66GQ Ch. 5 - For each of the following, define a system and its...Ch. 5 - Prob. 68GQ Ch. 5 - Use Appendix L to find the standard enthalpies of...Ch. 5 - You have a large balloon containing 1.0 mol of...Ch. 5 - Determine whether energy as heat is evolved or...Ch. 5 - Determine whether energy as heat is evolved or...Ch. 5 - Use standard enthalpies of formation to calculate...Ch. 5 - Which evolves more energy on cooling from 50 C to...Ch. 5 - You determine that 187 J of energy as heat is...Ch. 5 - Calculate the quantity of energy required to...Ch. 5 - You add 100.0 g of water at 60.0 C to 100.0 g of...Ch. 5 - Three 45-g ice cubes at 0 C are dropped into 5.00 ...Ch. 5 - Suppose that only two 45-g ice cubes had been...Ch. 5 - You take a diet cola from the refrigerator and...Ch. 5 - The standard molar enthalpy of formation of...Ch. 5 - Chloromethane, CH3Cl, a compound found throughout...Ch. 5 - Prob. 83GQ Ch. 5 - Camping stoves are fueled by propane (C3H8),...Ch. 5 - Prob. 85GQ Ch. 5 - Prob. 86GQ Ch. 5 - (a) Calculate the enthalpy change, rH, for the...Ch. 5 - You drink 350 mL of diet soda that is at a...Ch. 5 - Chloroform, CHCl3, is formed from methane and...Ch. 5 - Water gas, a mixture of carbon monoxide and...Ch. 5 - Using standard enthalpies of formation, verify...Ch. 5 - A piece of lead with a mass of 27.3 g was heated...Ch. 5 - A 192-g piece of copper is heated to 100.0 C in a...Ch. 5 - Insoluble AgCl(s) precipitates when solutions of...Ch. 5 - Insoluble PbBr2(s) precipitates when solutions of...Ch. 5 - The value of U for the decomposition of 7.647 g of...Ch. 5 - A bomb calorimetric experiment was run to...Ch. 5 - The meals-ready-to-eat (MREs) in the military can...Ch. 5 - On a cold day, you can warm your hands with a heat...Ch. 5 - Without doing calculations, decide whether each of...Ch. 5 - Prob. 102SCQ Ch. 5 - You want to determine the value for the enthalpy...Ch. 5 - Prepare a graph of specific heat capacities for...Ch. 5 - Prob. 105SCQ Ch. 5 - You are attending summer school and living in a...Ch. 5 - Prob. 107SCQ Ch. 5 - Prob. 108SCQ Ch. 5 - Prob. 109SCQ Ch. 5 - Peanuts and peanut oil are organic materials and...Ch. 5 - Isomers are molecules with the same elemental...Ch. 5 - Prob. 112SCQ Ch. 5 - Prob. 113SCQ Ch. 5 - A piece of gold (10.0 g, CAu = 0.129 J/g K) is...Ch. 5 - Methane, CH4, can be converted to methanol, which,...Ch. 5 - Calculate rH for the reaction 2 C(s) + 3 H2(g) + ...Ch. 5 - You have the six pieces of metal listed below,...Ch. 5 - Sublimation of 1.0 g of dry ice. CO2(s), forms...Ch. 5 - In the reaction of two moles of gaseous hydrogen...

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