Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 5, Problem 32PS
Nitrogen gas is confined in a cylinder with a movable piston under a constant pressure of 9.95 × 104 Pa. When 695 J of energy in the form of heat is transferred from the gas to the surroundings, its volume decreases by 1.88 L. What is the change in internal energy of the gas?
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Chapter 5 Solutions
Chemistry & Chemical Reactivity
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. 5.3 - Calculate the amount of energy necessary to raise...Ch. 5.3 - To make a glass of iced tea, you pour 250 mL of...Ch. 5.4 - Nitrogen gas (2.75 L) is confined in a cylinder...Ch. 5.5 - The combustion of ethane, C2H6, has an enthalpy...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. 5.7 - Use Hesss law to calculate the enthalpy change for...Ch. 5.7 - Calculate the standard enthalpy of combustion for...
Ch. 5.8 - The standard enthalpies of formation of KNO3(s)...Ch. 5.8 - Prob. 1.2ACPCh. 5.8 - The decomposition of nitroglycerin (C3H5N3O9)...Ch. 5.8 - Prob. 2.1ACPCh. 5.8 - Prob. 2.2ACPCh. 5.8 - Prob. 2.3ACPCh. 5.8 - Prob. 2.4ACPCh. 5.8 - Prob. 2.5ACPCh. 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. What...Ch. 5 - What quantity of energy, in joules, is required to...Ch. 5 - Ethanol, C2HsOH, boils at 78.29 C. How much...Ch. 5 - A 25.0-mL sample of benzene at 19.9 C was cooled...Ch. 5 - As a gas cools, it is compressed from 2.50 L to...Ch. 5 - A balloon expands from 0.75 L to 1.20 L as it is...Ch. 5 - A balloon does 324 J of work on the surroundings...Ch. 5 - As the gas trapped in a cylinder with a movable...Ch. 5 - When 745 J of energy in the form of heat is...Ch. 5 - The internal energy of a gas decreases by 1.65 kJ...Ch. 5 - A volume of 1.50 L of argon gas is confined in a...Ch. 5 - Nitrogen gas is confined in a cylinder with a...Ch. 5 - Nitrogen monoxide, a gas recently found to be...Ch. 5 - Calcium carbide, CaC2, is manufactured by the...Ch. 5 - Isooctane (2,2,4-trimethylpentane), one of the...Ch. 5 - Acetic acid. 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. 65GQCh. 5 - Prob. 66GQCh. 5 - For each of the following, define a system and its...Ch. 5 - Prob. 68GQCh. 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. 83GQCh. 5 - Camping stoves are fueled by propane (C3H8),...Ch. 5 - Prob. 85GQCh. 5 - Prob. 86GQCh. 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. 102SCQCh. 5 - You want to determine the value for the enthalpy...Ch. 5 - Prepare a graph of specific heat capacities for...Ch. 5 - Prob. 105SCQCh. 5 - You are attending summer school and living in a...Ch. 5 - Prob. 107SCQCh. 5 - Prob. 108SCQCh. 5 - Prob. 109SCQCh. 5 - Peanuts and peanut oil are organic materials and...Ch. 5 - Isomers are molecules with the same elemental...Ch. 5 - Prob. 112SCQCh. 5 - Prob. 113SCQCh. 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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- Nitrogen gas (2.75 L) is confined in a cylinder under constant atmospheric pressure (1.01 105 pascals). The volume of gas decreases to 2.10 L when 485 J of energy is transferred as heat to the surroundings. What is the change in internal energy of the gas?arrow_forwardWhen solid iron burns in oxygen gas (at constant pressure) to produce Fe2O3(s), 1651 kJ of heat is released for every 4 mol of iron burned. How much heat is released when 10.3 g Fe2O3(s) is produced (at constant pressure)? What additional information would you need to calculate the heat released to produce this much Fe2O3(s) if you burned iron in ozone gas, O3(g), instead of O2(g)?arrow_forwardGasohol, a mixture of gasoline and ethanol, C2H5OH, is used as automobile fuel. The alcohol releases energy in a combustion reaction with O2. C2H5OH(l)+3O2(g)2CO2(g)+3H2O(l) If 0.115 g ethanol evolves 3.62 kJ when burned at constant pressure, calculate the combustion enthalpy for ethanol.arrow_forward
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