Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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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,
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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...
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- The 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_forward9.46 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_forwardHow much heat is required to convert 135 g of ice at −15 °C into water vapor at 120 °C?arrow_forward
- What is the energy change when the temperature of 10.3 grams of solid graphite is decreased from 37.8 °C to 23.9 °C ?arrow_forwardWater has a heat of fusion (ΔHfus) of 6.01 kJ/mol. What is the change in energy of 5.0 g of water that freezes from the liquid phase to the solid phase? The molar mass of water is 18.01 g/mol.arrow_forwardGiven that a 10.0g sample of ice at 0.0 degrees celsius melts and then the resultant water proceeds to warm to 20.0 degrees celsius, there are two separate processes (dealing with the transfer of heat) that describe the occurence. What are those two processes? (Hint one involves the specific heat of water). Determine the delta H of the following reactions: CH4 (g) +2O2(g) → CO2 (g) +2H2O(l) CH4 (g) +2O2(g) → CO2 (g) +2H2O(g) What is the numerical difference between these two values? What is the only physical difference between the two reactions? What does the numerical difference represent, in terms of the physical difference between the two reactions? A 4.00g sample of rocket fuel was combusted in a bomb calorimeter according to the following reaction: 2CH6N2(l)+ 5O2(g) → 2N2(g) +2CO2(g) + 6H2O(l) The temperature of the surrounding calorimeter increased from 25.00C to 39.50 C and the heat capacity of the calorimeter was previously determined to be 7.794KJ/c. What is the…arrow_forward
- The heat of fusion of acetic acid, the principal organic component of vinegar, is 192 J/g. How much heat (in kilojoules) is required to melt 1.75 mol of solid acetic acid?arrow_forward54.73 g of water, H2O, 18.02 g/mol, was heated from -19.53 °C to 112.08 °C. The freezing and boiling point of water is 0.0 °C and 100. °C, respectively. The specific heat capacities of solid, liquid, and gaseous water is 2.03 J/(g*K), 4.18 J/(g*K), and 1.84 J/(g*K), respectively. The heat of fusion and vaporization of water is 6.01 kJ/mol and 40.67 kJ/mol, respectively. How much heat, in kJ, is required?arrow_forwardA 417.3 gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C. (heat capacity of solid = 2.96 J/g･°C; heat capacity of liquid = 1.75 J/g･°C; ∆Hfus = 8.04 kJ/mol; normal freezing point, Tf = 17.6 °C) How much energy (in kJ) is absorbed/released to heat the solid? How can I solve this problem, step by step?arrow_forward
- Energy Constants for H2O334 J/g = Heat of Fusion (Hf)2260 J/g = Heat of Vaporization (Hv)2.11 J/goC = Specific Heat Capacity of solid water4.18 J/goC = Specific Heat Capacity of liquid water2.00 =J/goC = Specific Heat Capacity of water vapor4. Calculate the amount of energy that is released when 400 grams of water vapor cools from 115oC to 100oC, and condenses into water at 100oC.arrow_forwardWater has a vaporization enthalpy of 2256 J/g, making it the largest of any molecular substance. For example, methane, CH4, has nearly the same molar mass, but its vaporization enthalpy is only 185 J/g. What explanation can be offered for this?arrow_forwardA 0.870-g piece of lithium metal is dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0°C. The reaction is 2 Li(s) + 2 H₂O(l) → 2 LiOH(aq) + H₂(g) ∆H = 446 kJ/mol Assuming no heat is lost to the surroundings, and that the final mixture has a specific heat capacity of 4.18 J/g･°C, calculate the final temperature in °C. The enthalpy of fusion for ice is 6.02 kJ/mol.arrow_forward
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