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 80E
Practice Exercise 1
When 0.243 g of Mg metal is combined with enough HCI to make 100 mL of solution in a constant-pressure calorimeter, the following reaction occurs:
Mg(s) + 2 HCl(aq)→MgCl2(aq)+H2(g)
If the temperature of the solution increases from 23.0 to 34.1 °C as a result of this reaction, calculate ΔH in kJ/mol Mg. Assume that the solution has a specific heat of 4-18 J/g-°C and a density of 1.00 g/mL.
- -19.1 kJ/mol
- -111 kJ/mol
- -191kJ/mol
- -464kJ/mol
- -961 kJ/mol
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
What mass of iron is produced if 48.5 kJ of heat are released according to the following equation?
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔrH° = – 24.8 kJ/mol
Express your answer to 3 significant figures.
Answer g F
Answer the following the questions given below
Given (Dissolution of Sodium Hydroxide)
Mass of Water = 200g
Initial Temperature of water = 20.0°C
Final Temperature of water = 26.49 °C
?water= 5430.832J
?dissolution= 5566.6028J
Mass of Solid NaOH= 5.0g
Moles of solid NaOH=0.12501 mol
Δ?of NaOH dissolution= -44.51 kJ/mol
Questions:
1.Is the dissolution of NaOH endothermic or exothermic? Justify your answer.
2.If you touch the sides of a beaker containing NaOH being dissolved, will it feel warm or cold to touch?
QUESTION 4
In the reaction: Ni(s) + 2CO(g) + 2PF3(g) → Ni(CO)2(PF3)2 (l), ∆Hf ° is zero for __________.
a
CO (g)
b
both CO(g) and PF3(g)
c
Ni (s)
d
Ni(CO)2(PF3)2 (l)
e
PF3
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
- Can someone verify my answers? I got: a) endothermic b)-1149.5 J c) 1149.5 J d)0.0117 mol e) 97704.05 J/molarrow_forwardQuestion 12 W A 5.00 g-sample of KOH(s) at 25.0°C was added to 100.0 g of H2O(1) at room temperature inside an insulated cup calorimeter, and the contents were stirred. After all the KOH(s) dissolved, the temperature of the solution had increased. Based on the information given, which of the following best justifies the claim that the dissolution of KOH(s) is a thermodynamically favorable process? The forces between the ions and the water molecules are strọnger than the forces between water molecules, thus AH 0. Therefore, AG 0. Therefore, AG 0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS > 0. Therefore. AG > 0. D The average kinetic energy of the particles increases, resulting in AH > 0. Also, the ions become more widely dispersed as KOH(s) dissolves, thus AS 0. esc Q Search or enter website name @ # $ % &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_forward
- Substance CaO (s) CO₂ (g) CaCO3 (s) What is AG for the reaction CaO(s) + CO₂(g) → CaCO³(s)? k AG°f (kJ/mol) -604 -394.4 -112.8arrow_forwardNeed help in chemistry problemarrow_forwardWhat type of reaction and how much energy is involved in a reaction of boron trichloride with hydrochloric acid? B2H6(g) +6Cl2(g) ⟷2BCl3(g) + 6HCl(g) ΔH= -755.4 kJ/mole Group of answer choices Exothermic with ΔH = -755.4 kJ/mole. Exothermic with ΔH = +755.4 kJ/mole. Endothermic with ΔH = -755.4 kJ/mole. Endothermic with ΔH = +0.001324 kJ/mole. Endothermic with ΔH = +755.4 kJ/mole.arrow_forward
- Search 11:00 PM Tue Jan 24 F Question 26.a of 28 Tap here or pull up for additional resources A 8.65 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. What is the total mass inside the calorimeter in grams? 2 a 1 4 7 +/-arrow_forwardPlease correct answer and don't use hand ratingarrow_forward#2 For each reaction, find the value of ΔSo. Report the value with the appropriate sign. (a) 3 NO2(g) + H2O(l) →2 HNO3(l) + NO(g) =____J/K (b) N2(g) + 3 F2(g) →2 NF3(g) =____J/K (c) C6H12O6(s) + 6 O2(g) →6 CO2(g) + 6 H2O(g) =____J/Karrow_forward
- According to the following reaction, how much energy is evolved during the reaction of 72.5 g B2H6 and 32.5 g of Cl2? B2H6(g) +6 Cl2(g)→→2 BCl3(g) + 6 HCl(g) ΔHo = -1396 kJ Question 5 options: 3660 kJ 237 kJ 639 kJ 1280 kJ 107 kJarrow_forwardQuestion 9.a of 9 Submit Consider the reaction Cl2(g) + Br2(g) → 2 BrCI(g) at 25 °C. Using the information in the table, determine AS for this reaction. Compound AS° (J/mol·K) Cl2 (g) 223.0 Br2 (g) 245.4 BrCI (g) 240.0 J/mol ·K 1 2 3 4 6. C 7 8 +/- x 10 0 Tap here or pull up for additional resources LOarrow_forwardPractice 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 andarrow_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