Chemistry: The Central Science (13th Edition)
13th Edition
ISBN: 9780321910417
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
Textbook Question
Chapter 13, Problem 81E
Practical exercise 2
When 50.0 mL of 0.100MAgNO3 and 50.0 mL of 0.100 M HCI are mixed in a constant-pressure calorimeter, the temperature of the mixture increases from 22.30 to 23.11 °C. The temperature increase is caused by the following reaction:
AgNO3(aq)
HC1(aq)→AgCI(s)+HNO3(aq)
Calculate ΔH 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.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Practice Exercise 1
When 0.243 g of Mg metal is combined with enough HCl to
make 100 mL of solution in a constant-pressure calorimeter,
the following reaction occurs:
Mg(s) +2 HCI(aq) MgCl2(aq) + H2(8)
If the temperature of the solution increases from 23.0 to
34.1 °C as a result of this reaction, calculate AH in kJ/mol Mg.
Assume that the solution has a specific heat of 4.18 J/g-°C and
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.
What is the change in enthalpy (in kJ mol⁻¹) for the following reaction
Cl₂(g) + 2LiF(s) ⇄ 2ClF(g) + 2Li(s)
Question 1 options:
1)
-1064 kJmol⁻¹
2)
1123 kJmol⁻¹
3)
-1123 kJmol⁻¹
4)
1064 kJmol⁻¹
5)
199.65 kJmol⁻¹
How much heat is needed to convert 15.0 grams of BCl₃(s) at -107.4˚C to BCl₃(g) at 12.4˚C?
Question 2 options:
1)
0.269 kJ
2)
4.95 kJ
3)
1.64 kJ
4)
3.04 kJ
5)
16.4 kJ
This was all of the information given to us. Thank you!
Chapter 13 Solutions
Chemistry: The Central Science (13th Edition)
Ch. 13.3 - The labels have fallen off three bottles...Ch. 13.3 - Explain how a redox reaction involves electrons in...Ch. 13.3 - Prob. 13.2.1PECh. 13.3 - Prob. 13.2.2PECh. 13.4 -
4.11 Which data set, of the two graphed here,...Ch. 13.4 - You are titrating an acidic solution with a basic...Ch. 13.4 - State whether each of the following statements is...Ch. 13.4 - State whether each of the following statements is...Ch. 13.4 -
4.15 We have learned in this chapter that many...Ch. 13.4 - Prob. 13.5.2PE
Ch. 13.4 -
4.17 Specify what ions are present in solution...Ch. 13.4 - Prob. 13.6.2PECh. 13.5 - Prob. 13.7.1PECh. 13.5 - Acetone. CH3COCH3, is a nonelectrolyte;...Ch. 13.5 -
4.21 Using solubility guidelines, predict whether...Ch. 13.5 - Prob. 13.8.2PECh. 13.5 - Prob. 13.9.1PECh. 13.5 - Prob. 13.9.2PECh. 13.5 -
4 3 Use the molecular representations shown here...Ch. 13.5 - The concept of chemical equilibrium is very...Ch. 13.5 -
4 5 You are presented with a white solid and told...Ch. 13.5 - Which of the following ions will always be a...Ch. 13 - Which element is oxidized, and which is reduced in...Ch. 13 - Which of the following are redox reactions? For...Ch. 13 - Prob. 2ECh. 13 - Prob. 3ECh. 13 - Prob. 4ECh. 13 - Prob. 5ECh. 13 - The solubility of Xe in water at 1 atm pressure...Ch. 13 - The coinage metals (Group 1B) copper, silver, and...Ch. 13 - Prob. 8ECh. 13 - The contents of the closed box in each of the...Ch. 13 - An aqueous solution of an unknown solute is tested...Ch. 13 -
4.42 Because the oxide ion is basic, metal oxides...Ch. 13 - Prob. 12ECh. 13 -
4.44 As K20 dissolves in water, the oxide ion...Ch. 13 - True or false: If a substance is oxidized, it is...Ch. 13 - Prob. 15ECh. 13 - Which region of the periodic table shown here...Ch. 13 - Determine the oxidation number of sulfur in each...Ch. 13 - Determine the oxidation number for the indicated...Ch. 13 - Determine the oxidation number for the indicated...Ch. 13 - Write balanced molecular and net ionic equations...Ch. 13 - Using the activity series (Table 4.5), write...Ch. 13 - The enthalpy of solution of KBr in water is about...Ch. 13 - Prob. 23ECh. 13 -
4.58 The following reactions (note that the...Ch. 13 - Is the concentration of a solution an intensive or...Ch. 13 - Prob. 26ECh. 13 - Calculate the molarity of a solution that contains...Ch. 13 -
4.62
Calculate the molarity of a solution made by...Ch. 13 - Prob. 29ECh. 13 -
4.66 The average adult male has a total blood...Ch. 13 -
4.67
How many grams of ethanol, CH2CH2OH should...Ch. 13 - Prob. 32ECh. 13 - Which will have the highest concentration of...Ch. 13 - Prob. 34ECh. 13 - Prob. 35ECh. 13 - 13.36 Explain why pressure substantially affects...Ch. 13 - Prob. 37ECh. 13 - Prob. 38ECh. 13 - Prob. 39ECh. 13 - Prob. 40ECh. 13 - Prob. 41ECh. 13 - Prob. 42ECh. 13 - Prob. 43ECh. 13 - Prob. 44ECh. 13 - Some sulfuric acid is spilled on a lab bench You...Ch. 13 -
4.84 The distinctive odor of vinegar is due to...Ch. 13 - A 4.36-g sample of an unknown alkali metal...Ch. 13 -
4.86 An 8.65-g sample of an unknown group 2A...Ch. 13 - A solution of 100.0 mL of 0.200 M KOH is mixed...Ch. 13 - A 1.248-9 sample of limestone rock is pulverized...Ch. 13 - 4.91 Uranium hexafluoride, UF6, is processed to...Ch. 13 - The accompanying photo shows the reaction between...Ch. 13 - Prob. 53ECh. 13 -
4.94 You choose to investigate some of the...Ch. 13 -
4 95 Antacids are often used to relieve pain and...Ch. 13 -
4 96 The commercial production of nitric acid...Ch. 13 - Consider the following reagents: zinc, copper,...Ch. 13 - 98 Bronze is a solid solution of Cu(s) and Sn(s);...Ch. 13 - Prob. 59ECh. 13 - Tartaric acid. H2C4H4O6, has two acidic hydrogens....Ch. 13 - Prob. 61ECh. 13 - A solid sample of Zn(OH)2 is added to 0.350 L of...Ch. 13 - Prob. 63ECh. 13 - Prob. 64ECh. 13 - Prob. 65ECh. 13 - A fertilizer railroad car carrying 34,300 gallons...Ch. 13 - Prob. 67ECh. 13 - Prob. 68ECh. 13 - Prob. 69ECh. 13 - Prob. 70ECh. 13 -
4.115 Federal regulations set an upper limit of...Ch. 13 - A mixture of gases A2 and B2 are introduced to a...Ch. 13 - Practice Exercise 2 Calculate the change in the...Ch. 13 - A solid sample of Zn(OH)2 is added to 0.350 L of...Ch. 13 -
Practice Exercise 2
Calculate the work, in J, if...Ch. 13 - Practice Exercise 1 A chemical reaction that gives...Ch. 13 - Prob. 77ECh. 13 - Prob. 78ECh. 13 - Prob. 79ECh. 13 - Practice Exercise 1 When 0.243 g of Mg metal is...Ch. 13 - Practical exercise 2 When 50.0 mL of 0.100MAgNO3...Ch. 13 - Prob. 82ECh. 13 - Prob. 83ECh. 13 - Prob. 84ECh. 13 - Prob. 85ECh. 13 - Calculate H for the reaction C(s)+...Ch. 13 - Prob. 87ECh. 13 - Prob. 88ECh. 13 - Prob. 89ECh. 13 - Prob. 90ECh. 13 - Prob. 91AECh. 13 - Prob. 92AECh. 13 -
Use the average bond enthalpies in Table 5.4 to...Ch. 13 - Prob. 94AECh. 13 - Prob. 95AECh. 13 - One of the important ideas of thermodynamics is...Ch. 13 - Two positively charged spheres, each with a charge...Ch. 13 - SI The accompanying photo shows a pipevine...Ch. 13 - Consider the accompanying energy diagram. Does...Ch. 13 - Write balanced net ionic equations for the...Ch. 13 -
4.27 Separate samples of a solution of an unknown...Ch. 13 - Prob. 102AECh. 13 - Prob. 103AECh. 13 - Prob. 104AECh. 13 - Prob. 105AECh. 13 - Prob. 106IECh. 13 - State whether each of the following statements is...Ch. 13 - State whether each of the following statements is...Ch. 13 - A textbook on chemical thermodynamics states, “The...Ch. 13 - Prob. 110IECh. 13 - Prob. 111IECh. 13 - Complete and balance the following molecular...Ch. 13 -
[13.113]At 35°C the vapor pressure of acetone,...Ch. 13 - Write balanced molecular and net ionic equations...
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
- Exercise The overall reaction in a commercial heat pack can be represented as 4Fe(s) + 30, (g)→ 2Fe,O, (s) AH = -1652 kJ How much heat is released when 4.00 moles of iron are reacted with excess 0,? How much heat is released when 1.00 mole of Fe,03 is produced? 4Fe(s) + 30, (g)→ 2Fe,O, (s) AH = -1652 kJ CLC CHM121 AUDI Page 7 Chapter 6: Thermochemistry How much heat is released when 1.00 g iron is reacted with excess O,?arrow_forward4. Consider the reaction 2 H2 (g) + O2 (g) → 2 H2O (g) having AH = -484 kJ/mol. Determine the magnitude of the heat exchanged with the surroundings when 4 mol of H2 and 4 mol of O2 react. (a) 484 kJ (b) 968 kJ (c) 1452 kJ (d) 1936 kJ (e) 2904 kJ (f) 3872 kJarrow_forwardA certain reaction has a AG° = 419.0 kJ at 298 K. The value of AS° for this reaction is 188.0 J/K. Above what temperature (in units of K) does this reaction become spontaneous? Assume that AH° and AS° do not depend on temperature. Answer: 2228.72 The correct answer is: 2526.7arrow_forward
- Course 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_forwardWhat would be the value of AS for the following reaction in J/K? A(g) + 2 B(g) - 5 C(g) + D(g) > S° (J/mol-K) A(g) B(g) C(g) D(g) 105.3 204.7 171.1 181.3 Your Answer: Answer unitsarrow_forwardConsider the reaction 4HCI(g) + O₂(g)- +2H₂O(g) + Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if the pressure of each gas is 13.76 mm Hg. ANSWER: 187.91 2Cl₂(g) kJ/molarrow_forward
- edu.co Question 6 of 14 What is the change in enthalpy in joules when 5.44 x 104mol of AgCI solid dissolves in water according to the following chemical equation: AgCI(s) Ag (aq) + C(aq) AH = 65.5 kJ 6.022 x 102 0.001 35.6 1000 0.0356 65.5 5.44 x 104 3.56 x 10° 0.00831 mol Ag g AgCl g Ag mol AgCI g Ch kJ mol CH search %23 72°Farrow_forwardHow much energy is evolved during the reaction of 15.50 g of Na, according to the reaction below? 2Na(s) + 2H₂O(l) → 2NaOH(aq) + H₂(g) AH°rxn= -367.5 kJ 247.8 kJ 482.9 kJ 119.0 kJ 4200 kJ Answer 123.9 kJ 753.3 kJarrow_forwardissue 7We want to express the equation below for the production of one mole of CH4(g) by specifying, in the equation, the amount of energy required. Al4C3(s) + 12H2O(l) → 4Al(OH)3(s) + 3CH4(g) ∆H = -1763.0 kJ a) 587.7 kJ on the product sideb) 587.7 kJ on the reactant sidec) 1763.0 kJ on the reactant sided) 1763.0 kJ on the product sidearrow_forward
- O3+ NO → O2 + NO2 is shown below: E (KJ) O3 + NO 200 11 Reaction Coordinate Which of the following are true? (Select all that apply.) ☐AE is positive. The value of AE in the presence of a catalyst would be smaller than -200 kJ. The value of Ea in the presence of a catalyst would be larger than 11.0 kJ. The magnitude of Ea for the reverse reaction is larger than 11.0 kJ. The energy of the products is lower than the energy of the reactants. O2 + NO2arrow_forwardGmail YouTube Maps Chem101 Update : E Reading List Question 13 of 23 Submit What is the change in enthalpy in joules when 5.44 x 10 mol of AgCl solid dissolves in water according to the following chemical equation: AgCl(s)→ Ag*(aq) + CI"(aq) AH = 65.5 kJ STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 0.00831 0.001 35.6 65.5 3.56 x 106 1 0.0356 1000 6.022 x 1023 5.44 x 104 mol Ag" g Ci kJ g Ag* mol CI" mol AgCl MacBook Air ロOロ F9 F10 F11 吕口 F3 F7 F8 F4 F5 F6arrow_forwardO THERMOCHEMISTRY Calculating a molar heat of reaction from formation enthalpies Using the table of standard formation enthalpies that you'll find under the ALEKS Data tab, calculate the reaction enthalpy of this reaction under standard conditions: 2 CH,OH(1)+3 O,(g)→2 CO,(g)+4H,0(1) Round your answer to the nearest kJ. kJ x10 Explanation Check 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility IMG-4405.jpg IMG-4404jpg Jmage_50376449.JPG image_50371073.JPG image_50353665.JPG Sha MacBook Air esc 80 DII F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 @ 23 $ & 1 2 3 4 5 7 80 IIarrow_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
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY