Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 6, Problem 101AE
It has been determined that the body can generate 5500 kJ of energy during one hour of strenuous exercise. Perspiration is the body’s mechanism for eliminating this heat. What mass of water would have to be evaporated through perspiration to rid the body of the heat generated during 2 hours of exercise? (The heat of vaporization of water is 40.6 kJ/mol.)
Expert Solution & Answer
Trending nowThis is a popular solution!
Chapter 6 Solutions
Chemistry
Ch. 6 - Define the following terms: potential energy,...Ch. 6 - Consider the following potential energy diagrams...Ch. 6 - What is the first law of thermodynamics? How can a...Ch. 6 - When a gas expands, what is the sign of w? Why?...Ch. 6 - What is the heat gained/released at constant...Ch. 6 - High-quality audio amplifiers generate large...Ch. 6 - Explain how calorimetry works to calculate H or E...Ch. 6 - What is Hesss law? When a reaction is reversed,...Ch. 6 - Define the standard enthalpy of formation. What...Ch. 6 - Objects placed together eventually reach the same...
Ch. 6 - What is meant by the term lower in energy? Which...Ch. 6 - A fire is started in a fireplace by striking a...Ch. 6 - Liquid water turns to ice. Is this process...Ch. 6 - Consider the following statements: ''Heat is a...Ch. 6 - Consider 5.5 L of a gas at a pressure of 3.0 atm...Ch. 6 - Consider 5.5 L of a gas at a pressure of 3.0 atm...Ch. 6 - What if energy was not conserved? How would this...Ch. 6 - Hesss law is really just another statement of the...Ch. 6 - In the equation w = P V, why is there a negative...Ch. 6 - Consider an airplane trip from Chicago, Illinois,...Ch. 6 - How is average bond strength related to relative...Ch. 6 - Assuming gasoline is pure C8H18(l), predict the...Ch. 6 - What is the difference between H and E?Ch. 6 - The enthalpy change for the reaction...Ch. 6 - Explain why oceanfront areas generally have...Ch. 6 - The equation for the fermentation of glucose to...Ch. 6 - Explain why H is obtained directly from coffee-cup...Ch. 6 - The enthalpy of combustion of CH4(g) when H2O (1)...Ch. 6 - The enthalpy change for a reaction is a state...Ch. 6 - Standard enthalpies of formation are relative...Ch. 6 - The combustion of methane can be represented as...Ch. 6 - Why is it a good idea to rinse your thermos bottle...Ch. 6 - Prob. 26QCh. 6 - What is incomplete combustion of fossil fuels? Why...Ch. 6 - Explain the advantages and disadvantages of...Ch. 6 - Prob. 29ECh. 6 - Which has the greater kinetic energy, an object...Ch. 6 - Consider the following diagram when answering the...Ch. 6 - A gas absorbs 45 kJ of heat and does 29 kJ of...Ch. 6 - Calculate E for each of the following. a. q = 47...Ch. 6 - A system undergoes a process consisting of the...Ch. 6 - If the internal energy of a thermodynamic system...Ch. 6 - Calculate the internal energy change for each of...Ch. 6 - A sample of an ideal gas at 15.0 atm and 10.0 L is...Ch. 6 - A piston performs work of 210. L atm on the...Ch. 6 - Consider a mixture of air and gasoline vapor in a...Ch. 6 - As a system increases in volume, it absorbs 52.5 J...Ch. 6 - A balloon filled with 39.1 moles of helium has a...Ch. 6 - One mole of H2O(g) at 1.00 atm and 100.C occupies...Ch. 6 - One of the components of polluted air is NO. It is...Ch. 6 - The reaction SO3(g)+H2O(l)H2SO4(aq) is the last...Ch. 6 - Are the following processes exothermic or...Ch. 6 - Are the following processes exothermic or...Ch. 6 - The overall reaction in a commercial heat pack can...Ch. 6 - Consider the following reaction:...Ch. 6 - Consider the combustion of propane:...Ch. 6 - Consider the following reaction:...Ch. 6 - For the process H2O(l) H2O(g) at 298 K and 1.0...Ch. 6 - For the following reactions at constant pressure,...Ch. 6 - Consider the substances in Table 7-1. Which...Ch. 6 - The specific heat capacity of silver is 0.24 J/Cg....Ch. 6 - A 500-g sample of one of the substances listed in...Ch. 6 - It takes 585 J of energy to raise the temperature...Ch. 6 - A 30.0-g sample of water at 280. K is mixed with...Ch. 6 - A biology experiment requires the preparation of a...Ch. 6 - A 5.00-g sample of aluminum pellets (specific heat...Ch. 6 - Hydrogen gives off 120. J/g of energy when burned...Ch. 6 - A 150.0-g sample of a metal at75.0C is added to...Ch. 6 - A 110.-g sample of copper (specific heat capacity...Ch. 6 - In a coffee-cup calorimeter, 50.0 mL of 0.100 M...Ch. 6 - In a coffee-cup calorimeter, 100.0 mL of 1.0 M...Ch. 6 - A coffee-cup calorimeter initially contains 125 g...Ch. 6 - In a coffee-cup calorimeter, 1.60 g NH4NO3 is...Ch. 6 - Consider the dissolution of CaCl2:...Ch. 6 - Consider the reaction...Ch. 6 - Quinone is an important type of molecule that is...Ch. 6 - The energy content of food is typically determined...Ch. 6 - The heat capacity of a bomb calorimeter was...Ch. 6 - The combustion of 0.1584 g benzoic acid increases...Ch. 6 - The enthalpy of combustion of solid carbon to form...Ch. 6 - Combustion reactions involve reacting a substance...Ch. 6 - Given the following data calculate H for the...Ch. 6 - Prob. 78ECh. 6 - The bombardier beetle uses an explosive discharge...Ch. 6 - Calculate H for the reaction...Ch. 6 - Given the following data...Ch. 6 - Given the following data...Ch. 6 - Give the definition of the standard enthalpy of...Ch. 6 - Write reactions for which the enthalpy change will...Ch. 6 - Use the values ofHf in Appendix 4 to calculate H...Ch. 6 - Use the values of Hf in Appendix 4 to calculate H...Ch. 6 - The Ostwald process for the commercial production...Ch. 6 - Calculate H for each of the following reactions...Ch. 6 - The reusable booster rockets of the space shuttle...Ch. 6 - The space shuttle Orbiter utilizes the oxidation...Ch. 6 - Consider the reaction...Ch. 6 - The standard enthalpy of combustion of ethene gas,...Ch. 6 - Water gas is produced from the reaction of steam...Ch. 6 - Syngas can be burned directly or converted to...Ch. 6 - Ethanol (C2H5OH) has been proposed as an...Ch. 6 - Methanol (CH3OH) has also been proposed as an...Ch. 6 - Some automobiles and buses have been equipped to...Ch. 6 - Acetylene (C2H2) and butane (C4H10) are gaseous...Ch. 6 - Prob. 99ECh. 6 - The complete combustion of acetylene, C2H2(g),...Ch. 6 - It has been determined that the body can generate...Ch. 6 - One way to lose weight is to exercise! Walking...Ch. 6 - Three gas-phase reactions were run in a...Ch. 6 - Nitrogen gas reacts with hydrogen gas to form...Ch. 6 - Combustion of table sugar produces CO2(g) and H2O(...Ch. 6 - Prob. 106AECh. 6 - A serving size of six cookies contains 4 g of fat,...Ch. 6 - Calculate H for the reaction...Ch. 6 - The enthalpy of neutralization for the reaction of...Ch. 6 - Given the following data: NO2(g) NO(g) + O(g)H =...Ch. 6 - If a student performs an endothermic reaction in a...Ch. 6 - In a bomb calorimeter, the reaction vessel is...Ch. 6 - The bomb calorimeter in Exercise 102 is filled...Ch. 6 - Consider the two space shuttle fuel reactions in...Ch. 6 - Consider the following equations:...Ch. 6 - Given the following data...Ch. 6 - At 298 K, the standard enthalpies of formation for...Ch. 6 - Using the following data, calculate the standard...Ch. 6 - A sample of nickel is heated to 99.8C and placed...Ch. 6 - Given: 2Cu2O(s) + O2(g) 4CuO(s)H = 288 kJ Cu2O(s)...Ch. 6 - Calculate H for each of the following reactions,...Ch. 6 - Consider a balloon filled with helium at the...Ch. 6 - In which of the following systems is(are) work...Ch. 6 - Which of the following processes are exothermic?...Ch. 6 - Consider the reaction...Ch. 6 - A swimming pool, 10.0 m by 4.0 m, is filled with...Ch. 6 - In a coffee-cup calorimeter, 150.0 mL of 0.50 M...Ch. 6 - Calculate H for the reaction...Ch. 6 - Which of the following substances have an enthalpy...Ch. 6 - Consider 2.00 moles of an ideal gas that are taken...Ch. 6 - For the process H2O(l)H2O(g) at 298 K and 1.0 atm,...Ch. 6 - The sun supplies energy at a rate of about 1.0...Ch. 6 - The best solar panels currently available are...Ch. 6 - On Easter Sunday, April 3, 1983, nitric acid...Ch. 6 - A piece of chocolate cake contains about 400...Ch. 6 - The standard enthalpies of formation for S(g),...Ch. 6 - You have a l.00-mole sample of water at 30.C and...Ch. 6 - A 500.0-g sample of an element at 195C is dropped...Ch. 6 - When 1.00 L of 2.00 M Na2SO4 solution at 30.0c is...Ch. 6 - The preparation of NO2(g) from N2(g) and O2(g) is...Ch. 6 - Nitromethane, CH3NO2, can be used as a fuel. When...Ch. 6 - A cubic piece of uranium metal (specific heat...Ch. 6 - 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 temperature of the cooling water as it leaves the hot engine of an automobile is 240 F. After it passes through the radiator it has a temperature of 175 F. Calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g oC.arrow_forwardHow much heat is absorbed by a 44.7-g piece of leadwhen its temperature increases by 65.4°C?arrow_forwardAlloys When a 58.8-g piece of hot alloy is placed in125 g of cold water in a calorimeter, the temperature ofthe alloy decreases by 106.1°C, while the temperature ofthe water increases by 10.5°C. What is the specific heat ofthe alloy?arrow_forward
- The specific heat of copper metal was determined by putting a piece of the metal weighing 35.4 g in hot water. The quantity of heat absorbed by the metal was calculated to be 47.0 J from the temperature drop of the water. What was the specific heat of the metal if the temperature of the metal rose 3.45C?arrow_forwardHow much would the temperature of 275 g of water increase if 36.5 U of heat were added?arrow_forwardEnthalpy a A 100.-g sample of water is placed in an insulated container and allowed to come to room temperature at 21C. To heat the water sample to 41C, how much heat must you add to it? b Consider the hypothetical reaction,2X(aq)+Y(l)X2Y(aq)being run in an insulated container that contains 100. g of solution. If the temperature of the solution changes from 21C to 31C, how much heat does the chemical reaction produce? How does this answer compare with that in part a? (You can assume that this solution is so dilute that it has the same heat capacity as pure water.) c If you wanted the temperature of 100. g of this solution to increase from 21C to 51C, how much heat would you have to add to it? (Try to answer this question without using a formula.) d If you had added 0.02 mol of X and 0.01 mol of Y to form the solution in part b, how many moles of X and Y would you need to bring about the temperature change described in part c. e Judging on the basis of your answers so far, what is the enthalpy of the reaction 2X(aq) + Y(l) X2Y(aq)?arrow_forward
- A piece of lead of mass 121.6 g was heated by an electrical coil. From the resistance of the coil, the current, and the Time the current flowed, it was calculated that 235 J of heat was added to the lead. The temperature of the lead rose from 20.4C to 35.5C. What is the specific heat of the lead?arrow_forward9.97 Suppose that the working fluid inside an industrial refrigerator absorbs 680 J of energy for every gram of material that vaporizes in the evaporator. The refrigerator unit uses this energy flow as part of a cyclic system to keep foods cold. A new pallet of fruit with a mass of 500 kg is placed in the refrigerator. Assume that the specific heat of the fruit is the same as that of pure water because the fruit is mostly water. Describe how you would determine the mass of the working fluid that would have to be evaporated to lower the temperature of the fruit by 15C. List any information you would have to measure or look up.arrow_forwardCalcium oxide (quicklime) reacts with water to produce calcium hydroxide (slaked lime). CaO(s)+H2O(l)Ca(OH)2(s);H=65.2kJ The heat released by this reaction is sufficient to ignite paper. How much heat is released when 28.6 g of calcium oxide reacts?arrow_forward
- 9.41 Under what conditions does the enthalpy change equal the heat of a process?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_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_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY