Basic Chemistry, Books a la Carte Edition (5th Edition)
5th Edition
ISBN: 9780134177090
Author: Timberlake, Karen C.
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 9, Problem 9.71AQAP
Each of the following is a reaction that occurs in the cells of the body. Identify which is exothermic and endothermic. (9.6)
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
When 3 moles of Fe2O3(s) react with H2(g) to form Fe3O4(s) and H2O(g) according to the following equation, 6.00 kJ of energy are evolved.3Fe2O3(s)
+
H2(g)2Fe3O4(s)
+
H2O(g)Is this reaction endothermic or exothermic?
What is the value of q?
Nitrogen oxide (NO) has been found to be a key component in many biological processes. It also can react with oxygen to give the brown gas NO2. When one mole of NO reacts with oxygen, 57.0 kJ of heat is evolved.A. Write the thermochemical equation for the reaction between one mole of nitrogen oxide and oxygen.B. Is the reaction exothermic or endothermic?C. What is H when 5.00 grams of nitrogen oxide reacts?D. How many grams of nitrogen oxide must react with an excess of oxygen to liberate ten kilojoules of heat?
A)When 1 mole of CO(g) reacts with Cl2(g) to form COCl2(g) according to the following equation, 108 kJ of energy are evolved.
CO(g)+Cl2(g)---->COCl2(g)
Is this reaction endothermic or exothermic?
What is the value of q? ---- kJ
B) When 2 moles of H2S(g) react with O2(g) to form H2O(g) and SO2(g) according to the following equation, 1.04×103 kJ of energy are evolved.
2H2S(g)+3O2(g)----->2H2O(g)+2SO2(g)
Is this reaction endothermic or exothermic?
What is the value of q? ------ kJ
Chapter 9 Solutions
Basic Chemistry, Books a la Carte Edition (5th Edition)
Ch. 9.1 - Calculate the total mass of the reactants and the...Ch. 9.1 - Calculate the total mass of the reactants and the...Ch. 9.2 - 9.3 Write all of the mole-mole factors for each of...Ch. 9.2 - Prob. 9.4QAPCh. 9.2 - Prob. 9.5QAPCh. 9.2 - Prob. 9.6QAPCh. 9.2 - Prob. 9.7QAPCh. 9.2 - Ammonia is produced by the reaction of nitrogen...Ch. 9.2 - Prob. 9.9QAPCh. 9.2 - Prob. 9.10QAP
Ch. 9.3 - Sodium reacts with oxygen to produce sodium oxide....Ch. 9.3 - Nitrogen gas reacts with hydrogen gas to produce...Ch. 9.3 - Prob. 9.13QAPCh. 9.3 - lron (III) oxide reacts with carbon to give iron...Ch. 9.3 - Nitrogen dioxide and water react to produce nitric...Ch. 9.3 - Calcium cyanamide, CaCN2 , reacts with water to...Ch. 9.3 - When solid lead(II) sulfide reacts with oxygen...Ch. 9.3 - When the gases dihydrogen sulfide and oxygen...Ch. 9.4 - Prob. 9.19QAPCh. 9.4 - A clock maker has 15 clock faces. Each clock...Ch. 9.4 - Prob. 9.21QAPCh. 9.4 - Prob. 9.22QAPCh. 9.4 - 9.23 For each of the following reactions, 20.0 g...Ch. 9.4 - For each of the following reactions. 20.0 g of...Ch. 9.4 - Prob. 9.25QAPCh. 9.4 - Prob. 9.26QAPCh. 9.5 - 9.27 Carbon disulfide is produced by the reaction...Ch. 9.5 - Prob. 9.28QAPCh. 9.5 - Prob. 9.29QAPCh. 9.5 - Prob. 9.30QAPCh. 9.5 - Prob. 9.31QAPCh. 9.5 - Prob. 9.32QAPCh. 9.6 - In an exothermic reaction, is the energy of the...Ch. 9.6 - Prob. 9.34QAPCh. 9.6 - Prob. 9.35QAPCh. 9.6 - Classify each of the following as exothermic or...Ch. 9.6 - Prob. 9.37QAPCh. 9.6 - Prob. 9.38QAPCh. 9.6 - Prob. 9.39QAPCh. 9.6 - Prob. 9.40QAPCh. 9.6 - Prob. 9.41QAPCh. 9.6 - Calculate the enthalpy change for the reaction...Ch. 9.6 - Prob. 9.43QAPCh. 9.6 - Prob. 9.44QAPCh. 9 - Prob. 9.45FUCh. 9 - Prob. 9.46FUCh. 9 - Prob. 9.47UTCCh. 9 - Prob. 9.48UTCCh. 9 - Prob. 9.49UTCCh. 9 - Prob. 9.50UTCCh. 9 - Prob. 9.51UTCCh. 9 - If green spheres represent chlorine atoms and red...Ch. 9 - Prob. 9.53UTCCh. 9 - Prob. 9.54UTCCh. 9 - When ammonia NH3 reacts with fluorine F2 , the...Ch. 9 - Gasohol is a fuel that contains ethanol C2H6O that...Ch. 9 - When hydrogen peroxide H2O2 is used in rocket...Ch. 9 - Propane gas, C3H8 , reacts with oxygen to produce...Ch. 9 - When 12.8 g of Na and 10.2 g of Cl2 react, what is...Ch. 9 - If 35.8 g of CH4 and 75.5 g of S react, how many...Ch. 9 - Pentane gas, C5H12 , reacts with oxygen to produce...Ch. 9 - When nitrogen dioxide NO2 from car exhaust...Ch. 9 - The gaseous hydrocarbon acetylene, C2H2 , used in...Ch. 9 - The equation for the decomposition of potassium...Ch. 9 - When 28.0 g of acetylene reacts with hydrogen....Ch. 9 - When 50.0 g of iron(III) oxide reacts with carbon...Ch. 9 - Nitrogen and hydrogen combine to form ammonia....Ch. 9 - Prob. 9.68AQAPCh. 9 - The equation for the reaction of nitrogen and...Ch. 9 - The equation for the reaction of iron and oxygen...Ch. 9 - Each of the following is a reaction that occurs in...Ch. 9 - Each of the following is a reaction that occurs in...Ch. 9 - Prob. 9.73CQCh. 9 - Prob. 9.74CQCh. 9 - Prob. 9.75CQCh. 9 - Prob. 9.76CQCh. 9 - Prob. 9.77CQCh. 9 - Prob. 9.78CQCh. 9 - Prob. 9.79CQCh. 9 - Prob. 9.80CQCh. 9 - Prob. 9.81CQCh. 9 - Prob. 9.82CQ
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
- 9.85 The figure below shows a "self-cooling" beverage can. The can is equipped with an outer jacket containing sodium carbonate (Na2CO3), which dissolves in water rapidly and endothermically: Na2CO3(s)2Na+(aq)+CO32(aq) H= 67.7 kJ The user adds water to the outer jacket, and the heat absorbed in the chemical reaction chills the drink. The can contains 200 g of drink, the jacket contains 55 g of Na2CO3, and 100 g of water is to be added. If the initial temperatures of the can and the water are both 32°C on a summer day, what is the coldest temperature that the drink can reach? The can itself has a heat capacity of 40 J/C Assume that the Na2CO3 solution and the drink both have the same heat capacity as pure water, 4.184 J g-l C-l, (HINT: Treat this like a calorimetry problem.)arrow_forwardHydrogen cyanide is used in the manufacture of clear plastics such as Lucite and Plexiglas. It is prepared from ammonia and natural gas (CH4). 2NH3(g)+3O2(g)+2CH4(g)2HCN(g)+6H2O(g) The reaction evolves 469 kJ of heat per mol of HCN formed. Is the reaction endothermic or exothermic? What is the value of q when 2 mol HCN forms?arrow_forwardHow many kJ of energy is produced* during the formation of 70.8 g of Fe, according to the reaction below? (*Report you answer as a positive value) Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) ΔH°rxn = -852 kJarrow_forward
- an important flavor component of vanilla extract is vanillin C8H8O3 molar mass = 152.15 g/mol when vanillin burns in a bomb calorimeter with a heat capacity of 8.60 kJ/°C the temp increases from 25.97°C to 31.18°C. if the heat of combustion of vanillin is -3760 kJ/mol what mass of vanillin (in g) was combusted? answer to two decimal placesarrow_forwardWhen 2 moles of HBr(g) react with cl2(g) to form HCl(g) and Br2(g) according to the following equation, 81.1 KJ of energy are evolved 2HBr(g) + cl2(g)------>2HCl(g)+ Br2(g) Is this reaction endothermic or exothermic?------ What is the value of q? ------KJ.arrow_forwardThe reaction of hydrogen chloride(g) with oxygen(g) to form water(g) and chlorine(g) proceeds as follows: 4 HCl(g) + O2(g) -----> 2 H2O(g) + 2 Cl2(g) When 13.7 grams of HCl(g) react with sufficient O2(g) , 10.7 kJ of energy are evolved .What is the value of H for the chemical equation given? ΔHrxn = kJarrow_forward
- When 1 mole of H2S(g) reacts with H2O(l) to form H2(g) and SO2(g) according to the following equation, 295 kJ of energy are absorbed.H2S(g) + 2H2O(l)3H2(g) + SO2(g) Is this reaction endothermic or exothermic? What is the value of q?arrow_forwardWhen copper(II) sulfate pentahydrate (CuSO4·5 H2O) is heated, it decomposes to the dehydrated form. The waters of hydration are released from the solid crystal and form water vapor. The hydrated form is medium blue, and the dehydrated solid is light blue. The balanced equation is CuSO4·5 H2O(s) --> CuSO4(s) + 5 H2O(g) *heat above the arrow If 5.32 g CuSO4·5 H2O is decomposed to CuSO4, predict the mass of the remaining light blue solid.arrow_forwardA calorimeter is charged with 57.9 mL of water at 25.0 °C. After a reaction takes place in the calorimeter, the water temperature is 26.4 °C. How much heat did the reaction produce, and was it exothermic or endothermic? (The density of water is 1.00 g/mL.)arrow_forward
- The reaction written below has a ΔH of +2,971 kJ 6CO2(g) + 6H2O(g) --> C6H12O6(g) +6O2(g) How much energy must be input into this reaction to make 93.087 grams of C6H12O6(g) ? (Input your answer in kJ, but do not include the units in your answer.)arrow_forwardA piece of parmesan cheese is burned in a soda can calorimeter, and heats up 0.235 kg of water by 2.85 °C. The calorimeter was calibrated and had a calorimetry constant of 8.50 kcal/kg･°C. Given that protein contains 4.00 kcal/g, calculate the mass in g of the protein contained in the parmesan. Assume that the cheese is composed primarily of protein.arrow_forwardThe combustion of ethane, C2H6, has an enthalpy change of -2857.4 KJ for the reaction as written below. Calculate ΔH° for the conbustion of 15.0 g of C2H6. 2 C2H6(g) +7 O2(g) → 4 CO2(g) + 6 H2O(g) ΔrH° = -2857.3 KJ/mol-rxnarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
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