EBK CHEMISTRY: AN ATOMS FIRST APPROACH
2nd Edition
ISBN: 9780100552234
Author: ZUMDAHL
Publisher: YUZU
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 7, Problem 76E
Write reactions for which the enthalpy change will be
a.
b. the standard enthalpy of combustion of liquid ethanol, C2H5OH(l).
c. the standard enthalpy of neutralization of sodium hydroxide solution by hydrochloric acid.
d.
e. the enthalpy of combustion of liquid benzene, C6H6(l).
f. the enthalpy of solution of solid ammonium bromide.
Expert Solution & Answer
Trending nowThis is a popular solution!
Chapter 7 Solutions
EBK CHEMISTRY: AN ATOMS FIRST APPROACH
Ch. 7 - Define the following terms: potential energy,...Ch. 7 - Consider the following potential energy diagrams...Ch. 7 - What is the first law of thermodynamics? How can a...Ch. 7 - When a gas expands, what is the sign of w? Why?...Ch. 7 - Prob. 5RQCh. 7 - High-quality audio amplifiers generate large...Ch. 7 - Explain how calorimetry works to calculate H or E...Ch. 7 - What is Hesss law? When a reaction is reversed,...Ch. 7 - Define the standard enthalpy of formation. What...Ch. 7 - Prob. 1ALQ
Ch. 7 - Prob. 2ALQCh. 7 - A fire is started in a fireplace by striking a...Ch. 7 - Liquid water turns to ice. Is this process...Ch. 7 - Prob. 5ALQCh. 7 - Prob. 6ALQCh. 7 - Consider 5.5 L of a gas at a pressure of 3.0 atm...Ch. 7 - Explain why oceanfront areas generally have...Ch. 7 - Hesss law is really just another statement of the...Ch. 7 - Prob. 10ALQCh. 7 - Prob. 11QCh. 7 - Prob. 12QCh. 7 - Assuming gasoline is pure C8H18(l), predict the...Ch. 7 - Prob. 14QCh. 7 - The enthalpy change for the reaction...Ch. 7 - For the reaction HgO(s)Hg(l)+12O2(g),H=+90.7KJ: a....Ch. 7 - Prob. 17QCh. 7 - The enthalpy change for a reaction is a state...Ch. 7 - Standard enthalpies of formation are relative...Ch. 7 - The combustion of methane can be represented as...Ch. 7 - Prob. 21QCh. 7 - Prob. 22QCh. 7 - Prob. 23QCh. 7 - Prob. 24QCh. 7 - Prob. 25ECh. 7 - Prob. 26ECh. 7 - Consider the following diagram when answering the...Ch. 7 - Consider the accompanying diagram. Ball A is...Ch. 7 - A gas absorbs 45 kJ of heat and does 29 kJ of...Ch. 7 - A system releases 125 kJ of heat while 104 kJ of...Ch. 7 - Calculate E for each of the following. a. q = 47...Ch. 7 - A system undergoes a process consisting of the...Ch. 7 - If the internal energy of a thermodynamic system...Ch. 7 - Calculate the internal energy change for each of...Ch. 7 - A sample of an ideal gas at 15.0 atm and 10.0 L is...Ch. 7 - Prob. 36ECh. 7 - Consider a mixture of air and gasoline vapor in a...Ch. 7 - As a system increases in volume, it absorbs 52.5 J...Ch. 7 - A balloon filled with 39.1 moles of helium has a...Ch. 7 - Prob. 40ECh. 7 - One of the components of polluted air is NO. It is...Ch. 7 - Prob. 42ECh. 7 - Are the following processes exothermic or...Ch. 7 - Are the following processes exothermic or...Ch. 7 - The overall reaction in a commercial heat pack can...Ch. 7 - Consider the following reaction:...Ch. 7 - Consider the combustion of propane:...Ch. 7 - Consider the following reaction:...Ch. 7 - Prob. 49ECh. 7 - The specific heat capacity of silver is 0.24 J/Cg....Ch. 7 - A 500-g sample of one of the substances listed in...Ch. 7 - Prob. 52ECh. 7 - A 30.0-g sample of water at 280. K is mixed with...Ch. 7 - A biology experiment requires the preparation of a...Ch. 7 - A 5.00-g sample of aluminum pellets (specific heat...Ch. 7 - Hydrogen gives off 120. J/g of energy when burned...Ch. 7 - Prob. 57ECh. 7 - A 110.-g sample of copper (specific heat capacity...Ch. 7 - In a coffee-cup calorimeter, 50.0 mL of 0.100 M...Ch. 7 - In a coffee-cup calorimeter, 100.0 mL of 1.0 M...Ch. 7 - A coffee-cup calorimeter initially contains 125 g...Ch. 7 - In a coffee-cup calorimeter, 1.60 g NH4NO3 is...Ch. 7 - Consider the dissolution of CaCl2:...Ch. 7 - Consider the reaction...Ch. 7 - The heat capacity of a bomb calorimeter was...Ch. 7 - The combustion of 0.1584 g benzoic acid increases...Ch. 7 - The enthalpy of combustion of solid carbon to form...Ch. 7 - Combustion reactions involve reacting a substance...Ch. 7 - Given the following data calculate H for the...Ch. 7 - Given the following data...Ch. 7 - Prob. 71ECh. 7 - Calculate H for the reaction...Ch. 7 - Given the following data...Ch. 7 - Given the following data...Ch. 7 - Give the definition of the standard enthalpy of...Ch. 7 - Write reactions for which the enthalpy change will...Ch. 7 - Prob. 77ECh. 7 - Use the values of Hf in Appendix 4 to calculate H...Ch. 7 - The Ostwald process for the commercial production...Ch. 7 - Calculate H for each of the following reactions...Ch. 7 - The reusable booster rockets of the space shuttle...Ch. 7 - The space shuttle Orbiter utilizes the oxidation...Ch. 7 - Consider the reaction...Ch. 7 - The standard enthalpy of combustion of ethene gas,...Ch. 7 - Water gas is produced from the reaction of steam...Ch. 7 - Prob. 86ECh. 7 - Prob. 87ECh. 7 - Prob. 88ECh. 7 - Some automobiles and buses have been equipped to...Ch. 7 - The complete combustion of acetylene, C2H2(g),...Ch. 7 - Prob. 91AECh. 7 - One way to lose weight is to exercise! Walking...Ch. 7 - Three gas-phase reactions were run in a...Ch. 7 - Nitrogen gas reacts with hydrogen gas to form...Ch. 7 - Combustion of table sugar produces CO2(g) and H2O(...Ch. 7 - Prob. 96AECh. 7 - Consider the following cyclic process carried out...Ch. 7 - Calculate H for the reaction...Ch. 7 - The enthalpy of neutralization for the reaction of...Ch. 7 - Prob. 100AECh. 7 - If a student performs an endothermic reaction in a...Ch. 7 - In a bomb calorimeter, the reaction vessel is...Ch. 7 - The bomb calorimeter in Exercise 102 is filled...Ch. 7 - Prob. 104AECh. 7 - Consider the following equations:...Ch. 7 - Prob. 106AECh. 7 - At 298 K, the standard enthalpies of formation for...Ch. 7 - Prob. 108AECh. 7 - A sample of nickel is heated to 99.8C and placed...Ch. 7 - Quinone is an important type of molecule that is...Ch. 7 - Calculate H for each of the following reactions,...Ch. 7 - Compare your answers from parts a and b of...Ch. 7 - Compare your answer from Exercise 72 of Chapter 3...Ch. 7 - Consider a balloon filled with helium at the...Ch. 7 - Prob. 115CWPCh. 7 - Prob. 116CWPCh. 7 - Prob. 117CWPCh. 7 - A swimming pool, 10.0 m by 4.0 m, is filled with...Ch. 7 - Prob. 119CWPCh. 7 - Calculate H for the reaction...Ch. 7 - Which of the following substances have an enthalpy...Ch. 7 - Consider 2.00 moles of an ideal gas that are taken...Ch. 7 - For the process H2O(l)H2O(g) at 298 K and 1.0 atm,...Ch. 7 - The sun supplies energy at a rate of about 1.0...Ch. 7 - Prob. 125CPCh. 7 - The standard enthalpies of formation for S(g),...Ch. 7 - Use the following standard enthalpies of formation...Ch. 7 - The standard enthalpy of formation for N2H4(g) is...Ch. 7 - The standard enthalpy of formation for NO(g) is...Ch. 7 - A piece of chocolate cake contains about 400...Ch. 7 - You have a l.00-mole sample of water at 30.C and...Ch. 7 - A 500.0-g sample of an element at 195C is dropped...Ch. 7 - A cubic piece of uranium metal (specific heat...Ch. 7 - On Easter Sunday, April 3, 1983, nitric acid...Ch. 7 - Using data from Chapter 2, calculate the change in...Ch. 7 - In Exercise 89 in Chapter 3, the Lewis structures...Ch. 7 - A gaseous hydrocarbon reacts completely with...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- The thermochemical equation for the burning of methane, the main component of natural gas, is CH4(g)+2O2(g)CO2(g)+2H2O(l)H=890kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = 890 kJ? (c) What is the enthalpy change when 1.00 g methane burns in an excess of oxygen?arrow_forwardA 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form MgCl2(aq) and H2(g). The temperature increases by 10.9 C as the magnesium reacts. Assume that the mixture has the same specific heat as water and a mass of 200 g. (a) Calculate the enthalpy change for the reaction. Is the process exothermic or endothermic? (b) Write the chemical equation and evaluate H.arrow_forwardWrite reactions for which the enthalpy change will be a. Hf for solid aluminum oxide. b. the standard enthalpy of combustion of liquid ethanol, C2H5OH(l). c. the standard enthalpy of neutralization of sodium hydroxide solution by hydrochloric acid. d. Hf for gaseous vinyl chloride, C2H3Cl(g). e. the enthalpy of combustion of liquid benzene, C6H6(l). f. the enthalpy of solution of solid ammonium bromide.arrow_forward
- A 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole-number coefficients, is 55.8 kJ. Both solutions are at 19.6C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, the specific heat of all solutions is the same as that of water, and volumes are additive.arrow_forwardA 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup calorimeter. As Ag2O(s) precipitates, the temperature of the solution increases from 23.78 C to 25.19 C. Assuming that the mixture has the same specific heat as water and a mass of 150 g, calculate the heat q. Is the precipitation reaction exothermic or endothermic?arrow_forwardA 29.1-mL sample of 1.05 M KOH is mixed with 20.9 mL of 1.07 M HBr in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole-number coefficients, is 55.8 kJ. Both solutions are at 21.8C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, and volumes are additive.arrow_forward
- What mass of acetylene, C2H2(g), must be burned to produce 3420 kJ of heat, given that its enthalpy of combustion is 1301 kJ/mol? Compare this with the answer to Exercise 5.91 and determine which substance produces more heat per gram.arrow_forwardWhen lightning strikes, the energy can force atmospheric nitrogen and oxygen to react to make NO: N2(g)+O2(g)2NO(g)H=+181.8kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = +181.8 kJ? (c) What is the enthalpy change when 3.50 g nitrogen is reacted with excess O2(g)?arrow_forwardUse data from Table 4.2 to calculate the standard combustion enthalpy for conversion of sulfur dioxide, SO2(g), to sulfur trioxide, SO3(g). Table 4.2 Selected Standard Formation Enthalpies, fH, at 25Carrow_forward
- In a bomb calorimeter, the reaction vessel is surrounded by water that must be added for each experiment. Since the amount of water is not constant from experiment to experiment, the mass of water must be measured in each case. The heat capacity of the calorimeter is broken down into two parts: the water and the calorimeter components. If a calorimeter contains 1.00 kg water and has a total heat capacity of 10.84 kJ/C, what is the heat capacity of the calorimeter components?arrow_forwardThe complete combustion of acetylene, C2H2(g), produces 1300. kJ of energy per mole of acetylene consumed. How many grams of acetylene must be burned to produce enough heat to raise the temperature of 1.00 gal water by 10.0c if the process is 80.0% efficient? Assume the density of water is 1.00 g/cm3arrow_forwardConsider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(OH)2 Assuming that the temperature of both solutions was initially 25.0C and that the final mixture has a mass of 400.0 g and a specific heat capacity of 4.18 J/C g, calculate the final temperature of the mixture.arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY