Chemistry: The Central Science (14th Edition)
14th Edition
ISBN: 9780134414232
Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 5.5, Problem 5.7.2PE
Practice Exercise 2
A 0.5865-g sample of lactic acid (HC3H5O3) reacts with oxygen in a calorimeter whose heat capacity is 4.812kJ/°C. The temperature increases from 23.10 to 24.95 °C. Calculate the heat of combustion of lactic acid
- per gram and
- per mole.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
A 150.9-g sample of a metal at 74.5°C is added to 150.9 g H2O at 15.1°C. The temperature of the water rises to 18.4°C. Calculate the
specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. The specific heat capacity of water is
4.18 J/°C•g.
Specific heat capacity
J/°C•9
Submit Answer
Try Another Version
3 item attempts remaining
Not Visited
Practice Exercise 1The coinage metals (Group 1B) copper, silver, and gold havespecific heats of 0.385, 0.233, and 0.129 J/g-K, respectively.Among this group, the specific heat capacity andthe molar heat capacity as the atomic weightincreases. (a) increases, increases (b) increases, decreases(c) decreases, increases (d) decreases, decreases
I Review I Constants I Periodic Table
Standard Enthalpy of Formation at 289 K
Substance
Formula AH; (kJ/mol)
Part A
Hydrogen
bromide
HBr(g) -36.26
Hypochlorous acid (HOCI) can decompose in the gas phase according
to the following balanced equation:
Hydrogen
chloride
HCI(g)
-92.30
2 HOCI(g) → 2 HCI(g) + O2(g)
AH = -31.0 kJ (T = 298 K, P = 1
atm)
Hydrogen fluoride HF(g)
-268.60
Using the enthalpy of this reaction and data in the following table,
calculate the standard enthalpy of formation for HOCI(g).
Hydrogen iodide
HI(g)
25.9
Methane
CH4(g)
-74.80
O -123 kJ/mol
+61.3 kJ/mol
Water vapor
H20(g)
-241.8
O -76.8 kJ/mol
-154 kJ/mol
+76.8 kJ/m
Submit
Request Answer
Provide Feedback
Next >
MacBook Air
K
Chapter 5 Solutions
Chemistry: The Central Science (14th Edition)
Ch. 5.2 - A mixture of gases A2 and B2 are introduced to a...Ch. 5.2 - Practice Exercise 2 Calculate the change in the...Ch. 5.3 - A solid sample of Zn(OH)2 is added to 0.350 L of...Ch. 5.3 -
Practice Exercise 2
Calculate the work, in J, if...Ch. 5.3 - Practice Exercise 1 A chemical reaction that gives...Ch. 5.3 - Prob. 5.3.2PECh. 5.4 - Prob. 5.4.1PECh. 5.4 - Prob. 5.4.2PECh. 5.5 - The coinage metals (Group 1B) copper, silver, and...Ch. 5.5 - Prob. 5.5.2PE
Ch. 5.5 - Practice Exercise 1 When 0.243 g of Mg metal is...Ch. 5.5 - Practical exercise 2 When 50.0 mL of 0.100MAgNO3...Ch. 5.5 - Prob. 5.7.1PECh. 5.5 - Practice Exercise 2 A 0.5865-g sample of lactic...Ch. 5.6 - Prob. 5.8.1PECh. 5.6 - Prob. 5.8.2PECh. 5.6 - Calculate H for the reaction C(s)+...Ch. 5.6 - Prob. 5.9.2PECh. 5.7 - Prob. 5.10.1PECh. 5.7 - Prob. 5.10.2PECh. 5.7 - Prob. 5.11.1PECh. 5.7 - Prob. 5.11.2PECh. 5.7 -
Practice Exercise 1
Given 2SO2(g) + 02(g) —>...Ch. 5.7 - Prob. 5.12.2PECh. 5.8 - Use the average bond enthalpies in Table 5.41to...Ch. 5.8 -
Use the average bond enthalpies in Table 5.4 to...Ch. 5.9 - Prob. 5.14.1PECh. 5.9 - Prob. 5.14.2PECh. 5 - One of the important ideas of thermodynamics is...Ch. 5 - Two positively charged spheres, each with a charge...Ch. 5 - SI The accompanying photo shows a pipevine...Ch. 5 - Consider the accompanying energy diagram. Does...Ch. 5 - The contents of the closed box in each of the...Ch. 5 - Imagine that you are climbing a mountain. Is the...Ch. 5 - The diagram shows four states of a system, each...Ch. 5 - You may have noticed that when you compress the...Ch. 5 - Imagine a container placed in a tub of water, as...Ch. 5 - In the accompanying cylinder diagram, a chemical...Ch. 5 - Prob. 10ECh. 5 - Consider the two diagrams that follow. Based on...Ch. 5 - Consider the conversion of compound A into...Ch. 5 - What is the electrostatic potential energy (in...Ch. 5 - What is the electrostatic potential energy (in...Ch. 5 - The electrostatic force (not energy) of attraction...Ch. 5 - Use the equations given in Problem 5.15 to...Ch. 5 - A sodium ion, Na+, with a charge of 1.6 x 10-19 C...Ch. 5 - A magnesium ion, Mg2+, with a charge of 3.2 x...Ch. 5 - Identify the force present and explain whether...Ch. 5 - Identify the force present and explain whether...Ch. 5 - Which of the following cannot leave or enter a...Ch. 5 - Prob. 22ECh. 5 - According to the first law of thermodynamics, what...Ch. 5 - Write an equation that expresses the first law of...Ch. 5 - Calculate AB and determine whether the process is...Ch. 5 - For the following processes, calculate the change...Ch. 5 - A gas is confined to a cylinder fitted with a...Ch. 5 - Consider a system consisting of two oppositely...Ch. 5 - What is meant by the term state function? Give an...Ch. 5 - Indicate which of the following is independent of...Ch. 5 - During a normal breath, our lungs expand about...Ch. 5 - How much work (in J) is involved in a chemical...Ch. 5 - Why is the change in enthalpy usually easier to...Ch. 5 - Under what condition will the enthalpy change of a...Ch. 5 - Assume that the following reaction occurs at...Ch. 5 - Suppose that the gas-phase reaction 2NO(g) + 02(g)...Ch. 5 - A gas is confined to a cylinder under constant...Ch. 5 - A gas is confined to a cylinder under constant...Ch. 5 - The complete combustion of ethanol, C2H5OH(l), to...Ch. 5 - The decomposition of Ca(OH)2(s) into CaO(s) and...Ch. 5 - Ozone, 03(9), is a form of elemental oxygen that...Ch. 5 -
5.42 Without referring to tables, predict which...Ch. 5 - Consider the following reaction: 2 Mg(s) + 02(g)2...Ch. 5 -
544 Consider the following reaction:
2...Ch. 5 - When solutions containing silver ions and chloride...Ch. 5 - At one time, a common means of forming small...Ch. 5 -
5.47 Consider the combustion of liquid methanol,...Ch. 5 -
5.48 Consider the decomposition of liquid...Ch. 5 - 5.49
a What are the units of molar heat...Ch. 5 - Two solid objects, A and B, are placed in boiling...Ch. 5 - What is the specific heat of liquid water? What is...Ch. 5 -
5.52
a. Which substance in Table 5.2 requires...Ch. 5 - The specific heat of octane, C8H18(l), is 2.22...Ch. 5 -
6.54 Consider the data about gold metal in...Ch. 5 - When a 6-50-g sample of solid sodium hydroxide...Ch. 5 -
5.56
a. When a 4 25-g sample of solid ammonium...Ch. 5 - A 2.200-g sample of quinone (C5H402) is burned in...Ch. 5 -
8.68 A 1.800-g sample of phenol (C6H5OH) was...Ch. 5 - Under constant-volume conditions, the heat of...Ch. 5 -
5.60 Under constant-volume conditions, the heat...Ch. 5 -
5.61 Can you use an approach similar to Hess's...Ch. 5 -
5.62 Consider the following hypothetical...Ch. 5 - Calculate the enthalpy change for the reaction...Ch. 5 - From the enthalpies of reaction calculate H for...Ch. 5 - From the enthalpies of reaction Calculate H for...Ch. 5 - Given the data use Hess's law to calculate H for...Ch. 5 -
5.67
What is meant by the term standard...Ch. 5 - S
5.68
What is the value of the standard enthalpy...Ch. 5 - For each of the following compounds, write a...Ch. 5 - Write balanced equations that describe the...Ch. 5 - The following is known as the thermite reaction:...Ch. 5 -
5.72 Many portable gas heaters and grills use...Ch. 5 - Using values from Appendix C , calculate the...Ch. 5 -
5.74 Using values from Appendix C, calculate the...Ch. 5 - Complete combustion of 1 mol of acetone (C2H6O)...Ch. 5 - Calcium carbide (CaC2) reacts with water to form...Ch. 5 -
5.77 Gasoline is composed primarily of...Ch. 5 - Prob. 78ECh. 5 - Ethanol (C2H5OH) is blended with gasoline as an...Ch. 5 -
5.80 Methanol (CH3OH) is used as a fuel in race...Ch. 5 -
5.81 Without doing any calculations, predict the...Ch. 5 -
5.82 Without doing any calculations, predict...Ch. 5 - Use bond enthalpies in Table 5.4 Q to estimate for...Ch. 5 - Use bond enthalpies in Table 5.40 to estimate for...Ch. 5 - Use enthalpies of formation given in Appendix C to...Ch. 5 -
5.86
The nitrogen atoms in an N2 molecule are...Ch. 5 -
5.87 Consider the reaction 2H(g) + O2(g) ...Ch. 5 -
5.88 Consider the reaction H2(g) + I2(s) ...Ch. 5 -
5.89
What is meant by the term fuel value?
Which...Ch. 5 -
5.90
Which releases the most energy when...Ch. 5 -
5.91
A serving of a particular ready-to-serve...Ch. 5 -
5.92 A pound of plain M&M® candies contains 96 g...Ch. 5 -
5.93 The heat of combustion of fructose,...Ch. 5 -
5.94 The heat of combustion of ethanol,...Ch. 5 -
5.95 The standard enthalpies of formation of...Ch. 5 -
5.98 It is interesting to compare the ‘fuel...Ch. 5 - At the end of 2012, global population was about...Ch. 5 -
5.98 The automobile fuel called E85 consists of...Ch. 5 - The air bags that provide protection in...Ch. 5 -
5.100 An aluminum can of a soft drink is placed...Ch. 5 -
5.101 Consider a system consisting of the...Ch. 5 - A sample of gas is contained in a...Ch. 5 - Limestone stalactites and stalagmites are formed...Ch. 5 - Consider the systems shown in Figure 5.10. In one...Ch. 5 -
5.105 A house is designed to have passive solar...Ch. 5 -
5.108 A coffee-cup calorimeter of the type shown...Ch. 5 -
5.107
When a 0.235-9 sample of benzoic acid is...Ch. 5 -
5.108 Meals-ready-to-eat (MREs) are military...Ch. 5 - 5.109 Burning methane in oxygen can produce three...Ch. 5 - Prob. 110AECh. 5 -
5.111 From the following data for three...Ch. 5 - The hydrocarbons acetylene (C2H2) and benzene...Ch. 5 - Ammonia (NH3) boils at -33 °C; at this temperature...Ch. 5 -
5.114 Three common hydrocarbons that contain four...Ch. 5 -
5.115 A 201-lb man decides to add to his exercise...Ch. 5 -
5.116 TheSun supplies about 1.0 kilowatt of...Ch. 5 -
5.117 Itis estimated that the net amount of...Ch. 5 -
5.118 At 20 °C (approximately room temperature)...Ch. 5 - Suppose an Olympic diver who weighs 52.0 kg...Ch. 5 -
5.120 Consider the combustion of a single...Ch. 5 -
5.121 Consider the following unbalanced...Ch. 5 - Consider the following acid-neutralization...Ch. 5 -
5.123 Consider two solutions, the first being...Ch. 5 - The precipitation reaction between AgNO3(aq) and...Ch. 5 -
5.125 A sample of a hydrocarbon is combusted...Ch. 5 -
5.126 The methane molecule, CH4, has the geometry...Ch. 5 -
5.127 One of the best-selling light, or...
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
- Course dashboard A bomb calorimetry experiment is performed with xylose, C5H1005 (s), as the combustible substance. The data obtained are mass of xylose burned: 2.059g, heat capacity of calorimeter 4.728 kJ/ C, initial calorimeter temperature: 23.29°C; final calorimeter temperature 27.19°C. What is the heat of combustion of xylose, in kilojoules di per mole? aretle Lütfen birini seçin: O a. -2.38x103 kJ/mol b. -2.17x103 kJ/mol Uy O c. -5.64x10 kJ/mol Ka d. -1.82x103 kJ/mol O e. -1.34x103 kJ/molarrow_forwardCalculate the energy required to heat 1.80 kg of graphite from 0.7 °C to 23.7 °C. Assume the specific heat capacity of graphite under these conditions is -1 0.710 J-g K'. Round your answer to 3 significant digits. Explanation Check Pikacy Center 2021 McGraw Roserved Te of Lnearrow_forwardA scientist measures the standard enthalpy change for the following reaction to be 543.0 kJ : 2BRF3(g)- →Br2(g) + 3 F2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of Br2(g) is kJ/mol. Submit Answer Try Another Version 1 item attempt remainingarrow_forward
- Practice Exercise 2 When 50.0 mL of 0.100 M AGNO3 and 50.0 mL of 0.100 M HC1 are mixed in a constant-pressure calorimeter, the temperature of the mixture increases from 22.30 to 23.11 °C. The tempera- ture increase is caused by the following reaction: AgNO3(aq) + HCI(aq) AgCl(s) + HNO3(aq) - Calculate AH for this reaction in kJ/mol AgNO3, assuming that the combined solution has a mass of 100.0 g and a specific heat of 4.18 J/g-°C.arrow_forwardReview I Constants I Periodic Table Part A In the following experiment, a coffee-cup calorimeter containing 100 mL of H, 0 is used. The initial temperature of the calorimeter is 23.0 °C. If 3.50 g of CaCl, is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution AHoln of CaCl, is -82.8 kJ/mol. Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water: C, = 4.184 J/g °C. Express your answer with the appropriate units. > View Available Hint(s) HA Value Units Submit < Return to Assignment Provide Feedbackarrow_forwardA scientist measures the standard enthalpy change for the following reaction to be -773.2 kJ : 2C0(g) + 2 NO(g)- →2CO2(g) + N2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO2(g) is kJ/mol. Submit Answer Try Another Version 2 item attempts remainingarrow_forward
- The molar heat capacity of dimethylsulfoxide is 88.0 J/mok-K. What is the specific heat capacity of this substance in the units of J/g-K? Question 17 options: A) 88.0 B) 1.13 C) 4.89 D) 6.88×103 E) -88.0arrow_forwardExercise 9.42 Enhanced with Feedback and Hints MISSED THIS? Watch KCV 9.4, IWE 9.2; Read Section 9.4. You can click on the Review link to access the section in your e Text. Part A How much heat is required to warm 1.30 kg of sand from 30.0 °C to 100.0 °C? Express the heat in joules to three significant figures. » View Available Hint(s) ΑΣφ Jarrow_forwardCourse Contents Practice Questions Topic 15-06 Timer Notes Evaluate Feedback Print Info A block of an alloy of mass 35.0 g and at a temperature of 2.02 °C is placed in a calorimeter containing 46.0 g of dichlorobenzene at 86.26 °C. If the final temperature of the alloy and dichlorobenzene is 67.45 °C, calculate the specific heat (in 3/g/K) of the metal. The specific heat of dichlorobenzene is 1.13 1/g/K. Express your answer to three significant figures in scientific notation. Submit Answer Tries 0/99arrow_forward
- O THERMOCHEMISTRY Solving a basic calorimetry problem thermometer A sample of polystyrene, which has a specific heat capacity of 1.880 J'g .°c', is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The polystyrene sample starts off at 96.4 °C and the temperature of the water starts off at 16.0 °C insulated container When the temperature of the water stops changing it's 22.2 °C. The pressure remains constant at 1 atm. water Calculate the mass of the polystyrene sample. Be sure your answer is rounded to the correct number of significant digits. sample a calorimeter IIarrow_forward- Practice Exercise 1 If the heat of formation of H,O(1) is –286 kJ/mol, which of the following thermochemical equations is correct? (a) 2 H(g) + O(g) → H2O(1) (b) 2 H2(8) + O2(8) (c) H2(8) + O2(8) (d) H2(g) + O(g) → H2O(g) (e) H2O(1) AH = -286 kJ AH = -286 kJ → 2 H,O(1) H20(1) %3D AH = -286 kJ AH = -286 kJ - %3D H2(8) + O2(8) AH = -286 kJ - %3Darrow_forwardMacmillan Learning Question 13 of 13 > At constant volume, the heat of combustion of a particular compound is -3549.0 kJ/mol. When 1.561 g of this compoun (molar mass = 166.20 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter, including its content. by 4.467 °C. What is the heat capacity (calorimeter constant) of the calorimeter? calorimeter constant: OO HUAWEI P30 LEICA TRIPLE CAMERA Answer a 7:25 PM 11/20/2022 - kJarrow_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 LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
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