Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 12.3, Problem 3RC
Interpretation Introduction
Interpretation:
The lattice enthalpy of sodium iodide should be calculated.
Concept introduction:
The lattice enthalpy is calculated by using following method,
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
A 22.5-g sample of ice at 0.0°C is added to 100.0 g of warm water at 35.0°C, and the final temperature
of the mixture is 14.0°C. (a) How much heat (in Joules) is lost by the warm water? (b) How much heat
(in Joules) is absorbed by the melted ice when its temperature increases from 0.0°C to 14.0°C?
(c) How much heat is absorbed by ice during melting at 0.0°C?
(d) What is the enthalpy of fusion of ice in kJ/mol?
3.
(Specific heat of water =
4.184 J/(g.°C)
Given the information below, calculate the lattice enthalpy for MX(s), where M is a group 1 metal, and X is a group 17 element (standard state: X2(g)).
ΔfH°(MX) = -462 kJ mol−1 ΔsubH°(M) = 127 kJ mol−1 D(X2) = 442 kJ mol−1 IE1(M) = 480 kJ mol−1 Eeg1(X) = -142 kJ mol−1 Express your answer to four significant figures.
ΔlattH°(MX) = Answer kJ mol−1
The enthalpy of vaporization of CO2(l) is 9.8 kJ/mol. Would you expect the enthalpy of vaporization of CS2(l) to be 28 kJ/mol, 9.8 kJ/mol, or −8.4 kJ/mol? Discuss the plausibility of each of these answers.
Chapter 12 Solutions
Chemistry & Chemical Reactivity
Ch. 12.1 - (a) Determining an Atom Radius from Lattice...Ch. 12.1 - Prob. 1RCCh. 12.1 - Prob. 2RCCh. 12.2 - If an ionic solid has an fcc lattice of anions (X)...Ch. 12.2 - Potassium chloride has the same unit cell as NaCl....Ch. 12.2 - 1. The unit cell of silicon carbide. SiC is...Ch. 12.2 - If one edge of the silicon carbide unit cell is...Ch. 12.2 - Prob. 1QCh. 12.2 - Describe the unit cell of lithium (see Figure).Ch. 12.2 - Prob. 3Q
Ch. 12.2 - Prob. 4QCh. 12.3 - Prob. 1RCCh. 12.3 - Prob. 2RCCh. 12.3 - Prob. 3RCCh. 12.4 - Prob. 1RCCh. 12.5 - Prob. 1QCh. 12.5 - Prob. 2QCh. 12.5 - Prob. 3QCh. 12.5 - 1. Which of the following allotropes of carbon is...Ch. 12.5 - Prob. 2RCCh. 12.6 - Prob. 1RCCh. 12.6 - Suppose you wanted to cool 100. g of water from 20...Ch. 12.7 - Prob. 1RCCh. 12.7 - How many tin atoms are contained in the tetragonal...Ch. 12.7 - Prob. 2QCh. 12.7 - Prob. 3QCh. 12.7 - Prob. 4QCh. 12 - Outline a two-dimensional unit cell for the...Ch. 12 - Outline a two-dimensional unit cell for the...Ch. 12 - Prob. 3PSCh. 12 - Rutile, TiO2, crystallizes in a structure...Ch. 12 - Cuprite is a semiconductor. Oxide ions are at the...Ch. 12 - The mineral fluorite, which is composed of calcium...Ch. 12 - Calcium metal crystallizes in a face-centered...Ch. 12 - The density of copper metal is 8.95 g/cm3. If the...Ch. 12 - Potassium iodide has a face-centered cubic unit...Ch. 12 - A unit cell of cesium chloride is illustrated in...Ch. 12 - Predict the trend in lattice energy, from least...Ch. 12 - Prob. 12PSCh. 12 - To melt an ionic solid, energy must be supplied to...Ch. 12 - Which compound in each of the following pairs...Ch. 12 - Prob. 15PSCh. 12 - Prob. 16PSCh. 12 - Considering only the molecular orbitals formed by...Ch. 12 - Prob. 18PSCh. 12 - Prob. 19PSCh. 12 - Prob. 20PSCh. 12 - Prob. 21PSCh. 12 - Prob. 22PSCh. 12 - Prob. 23PSCh. 12 - Prob. 24PSCh. 12 - A diamond unit cell is shown here. Unit cell of...Ch. 12 - The structure of graphite is given in Figure...Ch. 12 - We have identified six types of solids (metallic,...Ch. 12 - Prob. 28PSCh. 12 - Classify each of the following materials as...Ch. 12 - Prob. 30PSCh. 12 - Benzene, C6H6, is an organic liquid that freezes...Ch. 12 - The specific heat capacity of silver is 0.235 J/g ...Ch. 12 - Prob. 33PSCh. 12 - Prob. 34PSCh. 12 - Prob. 35PSCh. 12 - If your air conditioner is more than several years...Ch. 12 - Sketch a phase diagram for O2 from the following...Ch. 12 - Tungsten crystallizes in the unit cell shown here....Ch. 12 - Silver crystallizes in a face-centered cubic unit...Ch. 12 - The unit cell shown here is for calcium carbide....Ch. 12 - The very dense metal iridium has a face-centered...Ch. 12 - Vanadium metal has a density of 6.11 g/cm3....Ch. 12 - Prob. 43GQCh. 12 - Prob. 44GQCh. 12 - Prob. 45GQCh. 12 - Consider the three types of cubic units cells. (a)...Ch. 12 - The solid-state structure of silicon is shown...Ch. 12 - The solid-state structure of silicon carbide is...Ch. 12 - Spinels are solids with the general formula AB2O4...Ch. 12 - Using the thermochemical data below and an...Ch. 12 - Prob. 51GQCh. 12 - Prob. 52GQCh. 12 - Prob. 53GQCh. 12 - Prob. 54GQCh. 12 - Prob. 55GQCh. 12 - Prob. 56GQCh. 12 - Like ZnS, lead(II) sulfide, PbS (commonly called...Ch. 12 - CaTiO3, a perovskite, has the structure below. (a)...Ch. 12 - Potassium bromide has the same lattice structure...Ch. 12 - Calculate the lattice energy of CaCl2 using a...Ch. 12 - Why is it not possible for a salt with the formula...Ch. 12 - Prob. 63SCQCh. 12 - Prob. 64SCQCh. 12 - Prob. 65SCQCh. 12 - Phase diagrams for materials that have allotropes...
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
- 9.46 The heat of fusion of pure silicon is 43.4 kJ/mol. How much energy would be needed to melt a 5.24-g sample of silicon at its melting point of 1693 K?arrow_forwardThe cooling effect of alcohol on the skin is due to its evaporation. Calculate the heat of vaporization of ethanol (ethyl alcohol), C2H5OH. C2H5OH(l)C2H5OH(g);H=? The standard enthalpy of formation of C2H5OH(l) is 277.7 kJ/mol and that of C2H5OH(g) is 235.1 kJ/mol.arrow_forwardAre changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?arrow_forward
- Calcium carbide, CaC2, is manufactured by reducing lime with carbon at high temperature. (The carbide is used in turn to make acetylene, an industrially important organic chemical.) Is the reaction endothermic or exothermic?arrow_forwardDefine the joule in terms of SI base units.arrow_forwardThe enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?arrow_forward
- Explain why water boils at higher temperature under higher pressure (pure substance saturation temperature depends on pressure). Use knowledge of energy and energy transferring at molecular or atomic level during the phase change of a substance. You do not need to show calculations. • (a) the amount of heat absorbed as 1 kg of saturated liquid water boils at 100°C. (b) the amount of heat released as 1 kg of saturated water vapor condenses. Is a >b, a=b, or aarrow_forwardFermentation of glucose produces ethyl alcohol and carbon dioxide;C 6H 12O 6(l) → 2 C 2H 5OH(l) + 2 CO 2(g)What is ΔH° rxn (in kilojoules) if 658.1 mL of CO 2 was collected over water at 12.00°C and 696.4 mm Hg? The vapor pressure of water at this temperature is 10.52 mm Hg. Species ΔH°f, kJ/mol C6H12O6(l) -1260 C2H5OH(l) -277.7 CO2(g) -393.5arrow_forwardHow much heat is required to convert 58.2g of liquid water at 15 °C to water vapor at 125 °C. (Use the constants given in the example above.) kJarrow_forward7. a) How much heat (in kJ) must be removed when cooling 155 g of benzene, C6H6, at 120.0°C to solid benzene at 5.48°C? Given for benzene: boiling point at 1 atm = 80.1 °C Melting point at 1 atm = 5.48°C Specific heat (I) = 1.74 J/ g x °C Specific heat (g) = 1.04 J/ g × °C Heat of fusion = 127 J/g Heat of vaporization = 395 J/g %3D %3D b) Nickel has a face-centered cubic unit cell. The density of nickel is 6.84 g/cm3. Calculate a value for the atomic radius of nickelarrow_forwardCalculate ΔU (in joules) for the vaporization of 1.00 g of H2O at 100.°C and 1.00 atm pressure. The Hvap of H2O is 2260 J/g. Assume perfect gas behavior. The density of H2O at 100°C is 0.9588 g/cm3.arrow_forward6.023 x 1023 Magnesium (Mg) has an HCP crystal structure and a density of 1.740 g/cm³. What is the volume of its unit cell in cubic meters? (Given: Atomic weight of Mg is 24.31 g/mole and N₁ atoms/mole) (a) 9.28 x 10-23 m³. (b) 9.28 x 10-26 m³ (c) 1.39 x 10-25 m³ (d) 1.39 x 10-28 m³ 2.arrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
Recommended textbooks for you
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher: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 Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
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: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Types of Matter: Elements, Compounds and Mixtures; Author: Professor Dave Explains;https://www.youtube.com/watch?v=dggHWvFJ8Xs;License: Standard YouTube License, CC-BY