Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
Chapter 12, Problem 17PS
Interpretation Introduction
Interpretation:
The molar enthalpy formation of lithium fluoride has to be calculated.
Concept introduction:
The molar enthalpy formation is calculated by using following method,
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
16).
Using the thermochemical data below calculate the lattice energy for the formation of Na₂O.
Na(s) → Na(g)
107.3 kJ/mol
Na(g) → Na (g) + 1 e
-
495.9 kJ/mol
-418 kJ/mol
249.1 kJ/mol
-141 kJ/mol
-1484.5 kJ/mol
2 Na(s) + O₂(g) →→→ Na₂O(s)
1/2 O₂(g) → 0(g)
O(g) + 1 e→O(g)
O(g) +1e0²(g)
Please answer question 17 part A and B
Consider the reaction 2 S(g) + 3 O2(g) → 2 SO3(g). Using the standard enthalpies of formation listed in Appendix G of your text and the bond energy of 498.4 kJ/mol in molecular oxygen, calculate the average sulfur-oxygen bond energy, in units of kJ/mol, in sulfur trioxide gas. The answer is not 380/381.
Chapter 12 Solutions
Chemistry & Chemical Reactivity
Ch. 12.1 - (a) Determining an Atom Radius from Lattice...Ch. 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. 12.6 - Prob. 1.1ACPCh. 12.6 - Describe the unit cell of lithium (see Figure).Ch. 12.6 - Prob. 1.3ACPCh. 12.6 - Prob. 1.4ACPCh. 12.6 - Prob. 2.1ACPCh. 12.6 - Prob. 2.2ACPCh. 12.6 - Prob. 2.3ACP
Ch. 12.6 - How many tin atoms are contained in the tetragonal...Ch. 12.6 - Prob. 3.2ACPCh. 12.6 - Prob. 3.3ACPCh. 12.6 - Prob. 3.4ACPCh. 12 - Outline a two-dimensional unit cell for the...Ch. 12 - Outline a two-dimensional unit cell for the...Ch. 12 - A portion of the crystalline lattice for potassium...Ch. 12 - The unit cell of silicon carbide, SiC, is...Ch. 12 - Prob. 5PSCh. 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. 14PSCh. 12 - To melt an ionic solid, energy must be supplied to...Ch. 12 - Which compound in each of the following pairs...Ch. 12 - Prob. 17PSCh. 12 - Prob. 18PSCh. 12 - Considering only the molecular orbitals formed by...Ch. 12 - Prob. 20PSCh. 12 - Prob. 21PSCh. 12 - Prob. 22PSCh. 12 - Prob. 23PSCh. 12 - Prob. 24PSCh. 12 - Prob. 25PSCh. 12 - Prob. 26PSCh. 12 - Prob. 27PSCh. 12 - Prob. 28PSCh. 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. 32PSCh. 12 - Classify each of the following materials as...Ch. 12 - Prob. 34PSCh. 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. 37PSCh. 12 - Prob. 38PSCh. 12 - Prob. 39PSCh. 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. 47GQCh. 12 - Prob. 48GQCh. 12 - Prob. 49GQCh. 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. 55GQCh. 12 - Prob. 56GQCh. 12 - Prob. 57GQCh. 12 - Prob. 58GQCh. 12 - Prob. 59GQCh. 12 - Prob. 60GQCh. 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. 67SCQCh. 12 - Prob. 68SCQCh. 12 - Prob. 69SCQCh. 12 - Phase diagrams for materials that have allotropes...
Knowledge Booster
Similar questions
- What is a driving force? Name two common and important driving forces, and give an example of each. What is entropy? Although the total energy of the universe is constant, is the entropy of the universe constant? What is a spontaneous process?arrow_forward2arrow_forwardCalculate the heat released when 1.735 L O2 with a density of 1.11 g/L at 25°C reacts with an excess of hydrogen to form liquid water at 25°C. The enthalpy of formation of liquid water is –285.8 kJ/mol. Heat released = kJarrow_forward
- Your roommate is having trouble understanding why solids form. He asks, “Why would atoms bond into solids rather than just floating freely with respect to each other?” To help him understand at least one type of bonding in solids, you decide to embark on an energy explanation. You show him a drawing of a primitive cell of a sodium chloride crystal, NaCl, or simple table salt. The drawing is shown in the picture below where the orange spheres and Na ions and blue spheres are Cl ions. Each ion has a charge of magnitude equal to the elementary charge e. The ions lie on the corners of a cube of side ‘d’. You explain to your roommate that the electrical potential energy is defined as zero when all eight charges are infinitely far apart from each other. Then you bring them together to form the crystal structure shown. (a) Evaluate the electric potential energy of the crystal as shown and (b) show that it is energetically favorable for such crystals to form.arrow_forwardThe flame in a torch used to cut metal is produced by burning acetylene (C2H2) in pure oxygen. Assuming the combustion of 1 mole of acetylene releases 1251 kJ of heat, what mass of acetylene is needed to cut through a piece of steel if the process requires 32.2 × 104 kJ of heat?arrow_forwardCalculate the lattice energy of ionic solid MX, given the following thermodynamic data: M(s) + X2(9) → MX(s) AHræn M(s) → M(g) AHrän= 88. kJ Bond energy of X2 = 196. kJ/mol lonization energy for M(s) = 485. kJ /mol Electron affinity of X = -281. kJ/mol AHrxn = -616. Enter your answer in decimal notation, rounded to the appropriate number of significant figures.arrow_forward
- A 8.22-g sample of solid calcium reacted in excess fluorine gas to give a 16g sample of pure solid CaF2. The heat given off in this reaction was 251 kJ at constant pressure. Given this information, what is the enthalpy of formation of CaF2(s)?arrow_forwardCalculate the heat of sublimation of PI3[PI3(s)→PI3(g)]. The standard heat of formation of PI3(s) is -24.7 kJ/mol and the PI bond energy in this molecule is 184 kJ/mol. The standard heat of formation of P(g) is 334 kJ/mol and that of I2(g) is 62 kJ/mol. The I2 bond energy is 151 kJ/mol.arrow_forwardUse heat of formation data from Appendix E to calculate ∆H ° for the following reaction:ClO2 (g) + O(g) → ClO(g) + O2(g)arrow_forward
- Calculate the lattice enthalpy for RbC1. You will need the following information: Species AfH°, kJ/mol Rb(g) RbCl(s) Cl(g) 80.9 - 435.4 121.3 Enthalpy of ionization for Rb(g) is 403.0 kJ/mol; electron attachment enthalpy for Cl(g) is −349.0 kJ/mol. Lattice enthalpy = kJ/molarrow_forwardConsider a hypothetical ionic compound AB (comprised of A+ and B-ions). Given the following enthalpy data and using a Born-Haber cycle calculation, predict AH lattice in kJ mol-¹. A(s) + B(s) → AB(s) A-H = -376 kJ mol-¹ A(s) → A(g) A-H = 107 kJ mol-¹ B(s) → B(g) AH = 105 kJ mol-¹ First ionization energy of A(g) = 500 kJ mol-¹ Electron affinity enthalpy of B(g) (exothermic) = -316 kJ mol-¹ Answer:arrow_forwardWhat is the enthalpy of formation of water under standard state conditions? (See Appendix I| of your textbook.) O-241.8 kJ/mol O -237.1 kJ/mol O-285.8 kJ/mol O-228.6 kJ/molarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning