Chemistry Atoms First2e
2nd Edition
ISBN: 9781947172647
Author: OpenStax
Publisher: OpenStax College
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Textbook Question
Chapter 9, Problem 37E
A serving of a breakfast cereal contains 3 g of protein, 18 g of carbohydrates, and 6 g of fat. What is the Calorie content of a serving of this cereal if the average number of Calories for fat is 9.1 Calories/g, for carbohydrates is 4.1 Calories/g, and for protein is 4.1 Calories/g?
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There are 48 pairs of students in the following table. Each pair has quantitatively determined the mass of taurine in a 250 mL can of the popular energy drink marketed as “Munster” using High Performance Liquid Chromatography (HPLC). The class results are presented below:
QUESTION: Calculate the measurement of uncertainty and provide the data in a spreadsheet table.
Mass of Taurine (mg)
Mass of Taurine (mg)
(Table continued)
152.01
152.23
151.87
151.45
154.11
152.64
152.98
153.24
152.88
151.45
153.49
152.48
150.68
152.33
151.52
153.63
152.48
151.68
153.17
153.40
153.77
153.67
152.34
153.16
152.57
153.02
152.86
151.50
151.23
152.57
152.72
151.54
146.47
152.38
152.44
152.54
152.53
152.54
151.32
152.87
151.24
153.26
152.02
152.90
152.87
151.49
152.46
152.58
Chapter 9 Solutions
Chemistry Atoms First2e
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...
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