Chemistry: Atoms First
18th Edition
ISBN: 9781938168154
Author: Richard Langley, Klaus Theopold, Paul Flowers
Publisher: OpenStax College
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 9, Problem 24E
A 0.500-g sample of KCI is added to 50.0 g of water in a calorimeter (Figure 9.12). If the temperature decreases by 1.05 °C, what is the approximate amount of heat involved in the dissolution of the KCI, assuming the specific heat of the resulting solution is 4.18 J/ g °C? Is the reaction exothermic or endothermic?
Figure 9.12 A simple calorimeter can be constructed from two polystyrene cups. A the mometer and stirrer extend through the cover into the reaction mixture.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
Chemistry: Atoms First
Ch. 9 - A burning match and a bonfire may have the same...Ch. 9 - Prepare a table identifying several energy...Ch. 9 - Explain the difference between heat capacity and...Ch. 9 - Calculate the heat capacity, in joules and in...Ch. 9 - Calculate the heat capacity, in joules and in...Ch. 9 - How much heat, in joules and in calories, must be...Ch. 9 - How much heat, in joules and in calories, is...Ch. 9 - How much would the temperature of 275 g of water...Ch. 9 - If 14.5 kJ of heat were added to 485 g of liquid...Ch. 9 - A piece of unknown substance weighs 44.7 g and...
Ch. 9 - A piece of unknown solid substance weighs 437.2 g....Ch. 9 - An aluminum kettle weighs 1.05 kg. (a) What is the...Ch. 9 - Most people find waterbeds uncomfortable unless...Ch. 9 - A 500-mL bottle of water at room temperature and a...Ch. 9 - Would the amount of heat measured for the reaction...Ch. 9 - Would the amount of heat absorbed by the...Ch. 9 - Would the amount of heat absorbed by the...Ch. 9 - How many milliliters of water at 23 C with a...Ch. 9 - How much will the temperature of a cup (180 g) of...Ch. 9 - A 45-g aluminum spoon (specific heat 0.88 J/g C)...Ch. 9 - The temperature of the cooling water as it leaves...Ch. 9 - A 70.0-g piece of metal at 80.0 C is placed in 100...Ch. 9 - If a reaction produces 1.506 kJ of heat, which is...Ch. 9 - A 0.500-g sample of KCI is added to 50.0 g of...Ch. 9 - Dissolving 3.0 g of CaCl2(s) in 150.0 g of water...Ch. 9 - When 50.0 g of 0.200 M NaCl(aq) at 24.1 C is added...Ch. 9 - The addition of 3.15 g of Ba(OH)28H2O to a...Ch. 9 - The reaction of 50 mL of acid and 50 mL of base...Ch. 9 - If the 3.21 g of NH4NO3 in Example 9.6 were...Ch. 9 - When 1.0 g of fructose, C6H12O6(s), a sugar...Ch. 9 - When a 0.740-g sample of trinitrotoluene (TNT),...Ch. 9 - One method of generating electricity is by burning...Ch. 9 - The amount of fat recommended for someone with a...Ch. 9 - A teaspoon of the carbohydrate sucrose (common...Ch. 9 - What is the maximum mass of carbohydrate in a 6-oz...Ch. 9 - A pint of premium ice cream can contain 1100...Ch. 9 - A serving of a breakfast cereal contains 3 g of...Ch. 9 - Which is the least expensive source of energy in...Ch. 9 - Explain how the heat measured in Example 9.5...Ch. 9 - Using the data in the check your learning section...Ch. 9 - Calculate the enthalpy of solution( H for the...Ch. 9 - Calculate H for the reaction described by the...Ch. 9 - Calculate the enthalpy of solution ( H for the...Ch. 9 - Although the gas used in an oxyacetylene torch...Ch. 9 - How much heat is produced by burning 4.00 moles of...Ch. 9 - How much heat is produced by combustion of 125 g...Ch. 9 - How many moles of isooctane must be burned to...Ch. 9 - What mass of carbon monoxide must be burned to...Ch. 9 - When 2.50 g of methane burns in oxygen, 125 kJ of...Ch. 9 - How much heat is produced when loo mL of 0.250 M...Ch. 9 - A sample of 0.562 g of carbon is burned in oxygen...Ch. 9 - Before the introduction of chlorofluorocarbons,...Ch. 9 - Homes may be heated by pumping hot water through...Ch. 9 - Which of the enthalpies of combustion in Table 9.2...Ch. 9 - Does the standard enthalpy of formation of H2O(g)...Ch. 9 - Joseph Priestly prepared oxygen in 1774 by heating...Ch. 9 - How many kilojoules of heat will be released when...Ch. 9 - How many kilojoules of heat will be released when...Ch. 9 - The following sequence of reactions occurs in the...Ch. 9 - Both graphite and diamond burn....Ch. 9 - From the molar heats of formation in Appendix G,...Ch. 9 - Which produces more heat?...Ch. 9 - Calculate H for the process Sb(s)+52Cl2(g)SbCl5(s)...Ch. 9 - Calculate H for the process...Ch. 9 - Calculate H for the process Hg2Cl2(s)2Hg(l)+Cl2(g)...Ch. 9 - Calculate H for the process Co3O4(s)3Co(s)+202(g)...Ch. 9 - Calculate the standard molar enthalpy of formation...Ch. 9 - Using the data in Appendix G, calculate the...Ch. 9 - Using the data in Appendix G, calculate the...Ch. 9 - The following reactions can be used to prepare...Ch. 9 - The decomposition of hydrogen peroxide, H2O2, has...Ch. 9 - Calculate the enthalpy of combustion of propane,...Ch. 9 - Calculate the enthalpy of combustion of butane,...Ch. 9 - Both propane and butane are used as gaseous fuels....Ch. 9 - The white pigment TiO2 is prepared by the reaction...Ch. 9 - Water gas, a mixture of H2 and CO2 is an important...Ch. 9 - In the early days of automobiles, illumination at...Ch. 9 - From the data in Table 9.2, determine which of the...Ch. 9 - The enthalpy of combustion of hard coal averages...Ch. 9 - Ethanol, C2H5OH, is used as a fuel for motor...Ch. 9 - Among the substances that react with oxygen and...Ch. 9 - How much heat is produced when 1.25 g of chromium...Ch. 9 - Ethylene, C2H2, a byproduct from the fractional...Ch. 9 - The oxidation of the sugar glucose, C6H12O6, is...Ch. 9 - Propane, C3H8, is a hydrocarbon that is commonly...Ch. 9 - During a recent winter month in Sheboygan,...Ch. 9 - Which bond in each of the following pairs of bonds...Ch. 9 - Using the bond energies in Table 9.3, determine...Ch. 9 - Using the bond energies in Table 9.3, determine...Ch. 9 - Draw a curve that describes the energy of a system...Ch. 9 - Explain why bonds occur at specific average bond...Ch. 9 - When a molecule can form two different structures,...Ch. 9 - How does the bond energy of HCl(g) differ from the...Ch. 9 - Using the standard enthalpy of formation data in...Ch. 9 - Using the standard enthalpy of formation data in...Ch. 9 - Using the standard enthalpy of formation data in...Ch. 9 - Using the standard enthalpy of formation data in...Ch. 9 - Complete the following Lewis structure by adding...Ch. 9 - Use the bond energy to calculate an approximate...Ch. 9 - Use principles of atomic structure to answer each...Ch. 9 - The lattice energy of LiF is 1023 kJ/mol, and the...Ch. 9 - For which of the following substances is the least...Ch. 9 - The reaction of a metal, M, with a halogen, X2,...Ch. 9 - The lattice energy of LiF is 1023 kJ/mol, and the...Ch. 9 - Which compound in each of the following pairs has...Ch. 9 - Which compound in each of the following pairs has...Ch. 9 - Which of the following compounds requires the most...Ch. 9 - Which of the following compounds requires the most...Ch. 9 - The lattice energy of KF is 794 kJ/mol, and the...
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 equation for the fermentation of glucose to alcohol and carbon dioxide is: C6H12O6(aq) 2C2H5OH(aq) + 2CO2(g) The enthalpy change for the reaction is 67 kJ. Is this reaction exothermic or endothermic? Is energy, in the form of heat, absorbed or evolved as the reaction occurs?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_forwardGraphite is burned in oxygen to give carbon monoxide and carbon dioxide. If the product mixture is 33% CO and 67% CO2 by mass, what is the heat from the combustion of 1.00 g of graphite?arrow_forward
- Which molecule, HF, HCl, HBr, or HI, has the strongest chemical bond?arrow_forwardInsoluble AgCl(s) precipitates when solutions of AgNO3(aq) and NaCl(aq) are mixed. AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) rH = ? To measure the energy evolved in this reaction, 250. mL of 0.16 M AgNO3(aq) and 125 mL of 0.32 M NaCl(aq) are mixed in a coffee-cup calorimeter. The temperature of the mixture rises from 21.15 C to 22.90 C. Calculate the enthalpy change for the precipitation of AgCl(s), in kJ/mol. (Assume the density of the solution is 1.0 g/mL and its specific heat capacity is 4.2 J/g K.)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_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_forwardThe 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).arrow_forwardA rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forward
- Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the experimenter used a calorimeter that was a poorer insulator than a coffee cup calorimeter? Explain your answer.arrow_forwardNitrogen monoxide, a gas recently found to be involved in a wide range of biological processes, reacts with oxygen to give brown NO2 gas. 2 NO(g) + O2(g) NO2(g)rH = 114.1 kJ/mol-rxn Is this reaction endothermic or exothermic? What is the enthalpy change if 1.25 g of NO is converted completely to NO2?arrow_forwardA 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_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningGeneral 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 by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: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 by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
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
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