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
Textbook Question
Chapter 13.2, Problem 1RC
Given the enthalpy of formation data below, calculate
∆fH° [LiOH(s)] = − 484.93 kJ/mol | ∆fH° [LiOH(aq)] = − 508.48 kJ/mol |
- (a) +23.55 kJ/mol
- (b) +993.41 kJ/mol
(c) −23.55 kJ/mol
(d) −993.41 kJ/mol
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Given the following thermodynamic data:
CO2(g)
+
2NH3(g)
→
CO(NH2)2(s)
+
H2O(l)
ΔH°298
=-133.3 kJ
ΔG°298
=-6.97 kJ
ΔH°f (kJ/mol)
-393.5
-46.11
-285.8
S° (J/mol K)
213.6
192.3
104.6
69.91
a) Determine ΔH⁰f for CO(NH2)2(s)
b) Determine K for the reaction at 298 K
c) Determine ΔS⁰ for the reaction in units of J/K
d) Determine ΔG if the pressure of CO2 is 0.450 bar and the pressure of NH3 is 0.650 bar
e) Determine K for the reaction at 250 K
What is the quantity of heat evolved at constant pressure when 30.5 g H2O(l) isformed from the combustion of H2(g) and O2(g)?H2(g) + O2(g) → H2O(l); ΔH° = –285.8 kJa. 5.92 × 10–3 kJ b. 285.8 kJc. 8.72 × 103 kJ d. 168 kJe. 4.84 × 102 kJ
Use the table below to determine ΔH for the following reactionN 2H 4(g) + H 2O(g) ↔ NH 2OH(g) + NH 3(g)
Bond Energies, kJ/mol
Single Bonds
H
C
N
O
S
F
Cl
Br
I
H
432
C
411
346
N
386
305
167
O
459
358
201
142
S
363
272
---
---
286
F
565
485
283
190
284
155
Cl
428
327
313
218
255
249
240
Br
362
285
243
201
217
249
216
190
I
295
213
---
201
---
278
208
175
149
Multiple Bonds
C=C
602
C=N
615
C=O
799
C≡C
835
C≡N
887
C≡O
1072
N=N
418
N=O
607
S=O (in SO2)
532
N≡N
942
O2
494
S=O (in SO3)
469
Chapter 13 Solutions
Chemistry & Chemical Reactivity
Ch. 13.1 - (a) If you dissolve 10.0 g (about one heaping...Ch. 13.1 - You dissolve 1.0 mol of urea (H2NCONH2) in 270 g...Ch. 13.1 - 2. The concentration of acetic acid, CH3CO2H, in a...Ch. 13.2 - Use the data in Table 13.1 to calculate the...Ch. 13.2 - Given the enthalpy of formation data below,...Ch. 13.3 - Prob. 1CYUCh. 13.3 - Prob. 1RCCh. 13.3 - If the headspace of a soda is 25 mL and the...Ch. 13.3 - Prob. 2QCh. 13.3 - Prob. 3Q
Ch. 13.3 - Prob. 4QCh. 13.4 - Assume you dissolve 10.0 g of sucrose (C12H22O11)...Ch. 13.4 - What quantity of ethylene glycol, HOCH2CH2OH, must...Ch. 13.4 - In the northern United States, summer cottages are...Ch. 13.4 - Bradykinin is a small peptide (9 amino acids; 1060...Ch. 13.4 - An aluminum-containing compound has the empirical...Ch. 13.4 - A 1.40-g sample of polyethylene, a common plastic,...Ch. 13.4 - Calculate the freezing point of 525 g of water...Ch. 13.4 - 1. Vapor pressure: Arrange the following aqueous...Ch. 13.4 - Prob. 2RCCh. 13.4 - Samples of each of the substances listed below are...Ch. 13.4 - Motor mass: Erythritol is a compound that occurs...Ch. 13.5 - Prob. 1RCCh. 13.5 - The blue line on the diagram illustrates the...Ch. 13.5 - How many theoretical plates are required to...Ch. 13.5 - Prob. 3QCh. 13.5 - The vapor pressure of pure heptane is 361.5 mm Hg...Ch. 13 - You dissolve 2.56 g of succinic acid, C2H4(CO2H)2,...Ch. 13 - You dissolve 45.0 g of camphor, C10H16O, in 425 mL...Ch. 13 - Prob. 3PSCh. 13 - Prob. 4PSCh. 13 - Prob. 5PSCh. 13 - Prob. 6PSCh. 13 - Prob. 7PSCh. 13 - Prob. 8PSCh. 13 - Hydrochloric acid is sold as a concentrated...Ch. 13 - Concentrated sulfuric acid has a density of 1.84...Ch. 13 - The average lithium ion concentration in seawater...Ch. 13 - Silver ion has an average concentration of 28 ppb...Ch. 13 - Which pairs of liquids will be miscible? (a) H2O...Ch. 13 - Acetone, CH3COCH3, is quite soluble in water....Ch. 13 - Prob. 15PSCh. 13 - Use the following data to calculate the enthalpy...Ch. 13 - You make a saturated solution of NaCl at 25 C. No...Ch. 13 - Some lithium chloride, LiCl, is dissolved in 100...Ch. 13 - Prob. 19PSCh. 13 - The Henrys law constant for O2 in water at 25 is...Ch. 13 - An unopened soda can has an aqueous CO2...Ch. 13 - Hydrogen gas has a Henrys law constant of 7.8 104...Ch. 13 - A sealed flask contains water and oxygen gas at 25...Ch. 13 - Butane, C4H10, has been suggested as the...Ch. 13 - A 35.0-g sample of ethylene glycol, HOCH2CH2OH, is...Ch. 13 - Urea, (NH2)2CO, which is widely used in...Ch. 13 - Pure ethylene glycol, HOCH2CH2OH, is added 2.00 kg...Ch. 13 - Pure iodine (105 g) is dissolved in 325 g of CCl4...Ch. 13 - Prob. 29PSCh. 13 - What is the boiling point of a solution composed...Ch. 13 - Prob. 31PSCh. 13 - Prob. 32PSCh. 13 - Prob. 33PSCh. 13 - Some ethylene glycol, HOCH2CH2OH, is added to your...Ch. 13 - You dissolve 15.0 g of sucrose, C12H22O11, in a...Ch. 13 - A typical bottle of wine consists of an 11%...Ch. 13 - Prob. 37PSCh. 13 - Estimate the osmotic pressure of human blood at 37...Ch. 13 - An aqueous solution containing 1.00 g of bovine...Ch. 13 - Calculate the osmotic pressure of a 0.0120 M...Ch. 13 - You add 0.255 g of an orange, crystalline compound...Ch. 13 - Butylated hydroxyanisole (BHA) is used in...Ch. 13 - Benzyl acetate is one of the active components of...Ch. 13 - Anthracene, a hydrocarbon obtained from coal, has...Ch. 13 - An aqueous solution contains 0.180 g of an...Ch. 13 - Aluminon, an organic compound, is used as a...Ch. 13 - Prob. 47PSCh. 13 - To make homemade ice cream, you cool the milk and...Ch. 13 - List the following aqueous solutions in order of...Ch. 13 - Arrange the following aqueous solutions in order...Ch. 13 - When solutions of BaCl2 and Na2SO4 are mixed, the...Ch. 13 - The dispersed phase of a certain colloidal...Ch. 13 - Phenylcarbinol is used in nasal sprays as a...Ch. 13 - (a) Which aqueous solution is expected to have the...Ch. 13 - Arrange the following aqueous solutions in order...Ch. 13 - Prob. 56GQCh. 13 - Dimethylglyoxime [DMG, (CH3CNOH)2] is used as a...Ch. 13 - A 10.7 m solution of NaOH has a density of 1.33...Ch. 13 - Concentrated aqueous ammonia has a molarity of...Ch. 13 - Prob. 60GQCh. 13 - If you want a solution that is 0.100 m in ions,...Ch. 13 - Consider the following aqueous solutions: (i) 0.20...Ch. 13 - (a) Which solution is expected to have the higher...Ch. 13 - The solubility of NaCl in water at 100 C is 39.1...Ch. 13 - Instead of using NaCl to melt the ice on your...Ch. 13 - The smell of ripe raspberries is due to...Ch. 13 - Hexachlorophene has been used in germicidal soap....Ch. 13 - The solubility of ammonium formate, NH4CHO2, in...Ch. 13 - How much N2 can dissolve in water at 25 C if the...Ch. 13 - Cigars are best stored in a humidor at 18 C and...Ch. 13 - An aqueous solution containing 10.0 g of starch...Ch. 13 - Prob. 72GQCh. 13 - Calculate the enthalpies of solution for Li2SO4...Ch. 13 - Water at 25 C has a density of 0.997 g/cm3....Ch. 13 - If a volatile solute is added to a volatile...Ch. 13 - A solution is made by adding 50.0 mL of ethanol...Ch. 13 - A 2.0% (by mass) aqueous solution of novocainium...Ch. 13 - A solution is 4.00% (by mass) maltose and 96.00%...Ch. 13 - The following table lists the concentrations of...Ch. 13 - A tree is 10.0 m tall. (a) What must be the total...Ch. 13 - Prob. 81GQCh. 13 - A compound is known to be a potassium halide, KX....Ch. 13 - Prob. 85GQCh. 13 - If one is very careful, it is possible to float a...Ch. 13 - A solution of benzoic acid in benzene has a...Ch. 13 - You dissolve 5.0 mg of iodine, I2, in 25 mL of...Ch. 13 - Prob. 89ILCh. 13 - In a police forensics lab, you examine a package...Ch. 13 - An organic compound contains carbon (71.17%),...Ch. 13 - Prob. 92ILCh. 13 - When sails of Mg2+, Ca2+, and Be2+ are placed in...Ch. 13 - Explain why a cucumber shrivels up when it is...Ch. 13 - Prob. 95SCQCh. 13 - A 100.-gram sample of sodium chloride (NaCl) is...Ch. 13 - Prob. 97SCQCh. 13 - Prob. 98SCQCh. 13 - Starch contains CC, CH, CO, and OH bonds....Ch. 13 - Prob. 100SCQCh. 13 - You have two aqueous solutions separated by a...Ch. 13 - Prob. 102SCQCh. 13 - Sodium chloride (NaCl) is commonly used to melt...Ch. 13 - Prob. 105SCQCh. 13 - Prob. 106SCQCh. 13 - Prob. 107SCQ
Additional Science Textbook Solutions
Find more solutions based on key concepts
2. Why shouldn’t you work in a laboratory by yourself?
The Organic Chem Lab Survival Manual: A Student's Guide to Techniques
The active ingredient in Tylenol and a host of other over-the-counter pain relievers is acetaminophen (C8H9NO2)...
Chemistry: Atoms First
Q2. Which statement best defines chemistry?
a. The science that studies solvents, drugs, and insecticides
b. Th...
Introductory Chemistry (6th Edition)
Write a Lewis formula for each of the following organic molecules: C2H3Cl (vinyl chloride: starting material fo...
Organic Chemistry - Standalone book
Determine the number of protons, neutrons, and electrons in the following atoms: a. a hydrogen atom that has a ...
General, Organic, and Biological Chemistry (3rd Edition)
What is the pH range for acidic solutions? For basic solutions?
Introduction to Chemistry
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
- What is the average bond energy in CO2? CO2(g) ΔH°f, = –393.5 kJ mol–1 CO(g) ΔH°f, = –110.5 kJ mol–1 C(g) ΔH°f, = +715 kJ mol–1 CO32–(aq) ΔH°f, = –676.3 kJ mol–1 O(g) ΔH°f, = +249.0 kJ mol–1 Question 5 options: 207 kJ mol–1 1607 kJ mol–1 804 kJ mol–1arrow_forwardC(s) → C(g), ΔH = +715 kJmol-1 Cl2(g) → 2Cl(g), ΔH = +242 kJmol-1 C(s) + 2Cl2(g) → CCl4(g), ΔH = -135.5 kJmol-1 Calculate the average bond dissociation enthalpy of a C-Cl bond.arrow_forwardFermentation of glucose produces ethyl alcohol and carbon dioxide;C 6H 12O 6(l) → 2 C 2H 5OH(l) + 2 CO 2(g) The vapor pressure of water at this temperature is 13.63 mm Hg. Species ΔH°f, kJ/mol C6H12O6(l) -1260 C2H5OH(l) -277.7 CO2(g) -393.5 What is ΔH° rxn (in kilojoules) if 319.0 mL of CO 2 was collected over water at 16.00°C and 720.2 mm Hg?arrow_forward
- What is the quantity of heat evolved at constant pressure when 30.5 g H2O(l) is formed from the combustion of H2(g) and O2(g)? H2(g) + (1/2) O2(g) → H2O(l); ΔH° = –285.8 kJ a. 8.72 × 10^3 kJ b. 168 kJ c. 4.84 × 10^2 kJ d. 5.92 × 10^–3 kJ e. 285.8 kJarrow_forwardCH3OH (l) + 3/2 O2 (g) → CO2 (g) + 2 H2O (l), ΔH = -726.4 KJ/mol C (graphite) + O2 (g) → CO2 (g), ΔH = - 393.5 KJ/mol H2 (g) + ½ O2 (g) → H2O (l), ΔH = - 285.8 KJ/mol Calculate the enthalpy of formation of methanol from its elements: C (graphite) + 2 H2 (g) + ½ O2 (g) → CH3OH (l)arrow_forwardWhat is the enthalpy change when 8.20 moles ammonium chloride form in the following equation? N2 (g) + 4 H2 (g) + Cl2 (g) --> 2 NH4Cl (s) Delta H = – 628.8 kJ a. – 2.58 x 103 kJ b. – 1.29 x 103 kJ c. + 314.4 kJ d. – 314.4 kJ e. – 628.8 kJ f. – 5.16 x 103 kJ g. none of these d. – 314.4 kJarrow_forward
- Using values from Appendix C of your textbook, calculate the value of AH° for each of the following reactions. (a) 2 HBr(g) H₂(g) + Br₂(9) ΔΗ° = 72.8 (b) Fe₂O3(s) + 6 HCI(g) = 2 FeCl3(s) + 3 H₂O(g) AHO = 187.46 ΔΗ° = -180.74 XkJ (c) 2 NO(g) = N₂(g) + O₂(g) ΔΗ° ; X KJ = (d) 2 HI(g) H₂(g) + I₂(g) ✓ KJ X kjarrow_forwardFind ΔE, ΔH, q, and w for the change in state of 1.0 mol H2O(l ) at 80 °C to H2O( g) at 110 °C. The heat capacity of H2O(l ) at = 75.3 J/mol K, heat capacity of H2O( g) = 25.0 J/mol K, and the heat of vaporization of H2O is 40.7 * 103 J/mol at 100 °C.arrow_forwardThe dissolution of a 19.7 g of a given ionic solid in enough water to form 128 mL of solution causes a temperature decrease of 15.3 ºC. The density of the solution is 1.00 g/mL and its specific heat capacity is 4.18 J/g-ºC. The molar mass of the ionic solid is 78.24 g/mol. What is ∆H for the dissolution of the ionic solid in kilojoules per mole (kJ/mol)?arrow_forward
- Phosphorus oxychloride (POCl3) is a chlorinating agent that is frequently used in organic chemistry to replace oxygen with chlorine. Given if ΔHfus = 34.3 kJ/mol and ΔSfus = 125 J/(mol·K), what is the melting point of POCl3?arrow_forwardUsing the equations H₂ (g) + F₂ (g) → 2 HF (g) ∆H° = -79.2 kJ/mol C (s) + 2 F₂ (g) → CF₄ (g) ∆H° = 141.3 kJ/mol Determine the enthalpy for the reaction C (s) + 4 HF (g) → CF₄ (g) + 2 H₂ (g). -don't prematurely round -I had gotten the answer 180.9 but it was wrongarrow_forward17. The enthalpy of formation for H20(g), CO2(g), and C2H5OH(1), in kJ/mol, are given as follows: DH;°[H2O(g)] = -241.8; DH;°[CO2(g)] = -393.5, and DH;°[C2H5OH(1)] = -277.6 How much energy is produced when 2.50 g of ethanol (C2H5OH) is completely burned? C2H5OH(I) + 3O2{g) 2CO2(g) + 3H20(g); --> (A) 19.4 kJ (B) 49.5 kJ (C) 97.1 kJ (D) 67.0 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