Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 5, Problem 5.47QE
Interpretation Introduction
Interpretation:
Change in enthalpy for reaction when
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
Chemistry: Principles and Practice
Ch. 5 - Why must the physical states of all reactants and...Ch. 5 - Why is chemical energy classified as a form of...Ch. 5 - What is the difference between the enthalpy of...Ch. 5 - Classify each process as exothermic or...Ch. 5 - Explain why the specific heat of the contents of...Ch. 5 - Prob. 5.6QECh. 5 - Define heat. What are its units? How does it...Ch. 5 - Prob. 5.8QECh. 5 - Prob. 5.9QECh. 5 - Prob. 5.10QE
Ch. 5 - Prob. 5.11QECh. 5 - Is the Sun exothermic or endothermic? Is it any...Ch. 5 - Under what circumstances is the heat of a process...Ch. 5 - Prob. 5.14QECh. 5 - Prob. 5.15QECh. 5 - Prob. 5.16QECh. 5 - Prob. 5.17QECh. 5 - Prob. 5.18QECh. 5 - Prob. 5.19QECh. 5 - Prob. 5.20QECh. 5 - Prob. 5.21QECh. 5 - Prob. 5.22QECh. 5 - Prob. 5.23QECh. 5 - Prob. 5.24QECh. 5 - Prob. 5.25QECh. 5 - Prob. 5.26QECh. 5 - Prob. 5.27QECh. 5 - Prob. 5.28QECh. 5 - Prob. 5.29QECh. 5 - Prob. 5.30QECh. 5 - Prob. 5.31QECh. 5 - A chemical reaction occurs and absorbs 64.7 cal....Ch. 5 - The enthalpy change for the following reaction is...Ch. 5 - Prob. 5.34QECh. 5 - The thermochemical equation for the burning of...Ch. 5 - When lightning strikes, the energy can force...Ch. 5 - One step in the manufacturing of sulfuric acid is...Ch. 5 - If nitric acid were sufficiently heated, it can be...Ch. 5 - Prob. 5.39QECh. 5 - Prob. 5.40QECh. 5 - Prob. 5.41QECh. 5 - The combustion of 1.00 mol liquid methyl alcohol...Ch. 5 - Another reaction that is used to propel rockets is...Ch. 5 - Prob. 5.44QECh. 5 - Prob. 5.45QECh. 5 - Prob. 5.46QECh. 5 - Prob. 5.47QECh. 5 - Prob. 5.48QECh. 5 - Prob. 5.49QECh. 5 - Prob. 5.50QECh. 5 - The enthalpy change when 1 mol methane (CH4) is...Ch. 5 - Prob. 5.52QECh. 5 - Prob. 5.53QECh. 5 - How much energy is required to raise the...Ch. 5 - How much heat, in kilojoules, must be removed to...Ch. 5 - Prob. 5.56QECh. 5 - Prob. 5.57QECh. 5 - Prob. 5.58QECh. 5 - Prob. 5.59QECh. 5 - Prob. 5.60QECh. 5 - When 7.11 g NH4NO3 is added to 100 mL water, the...Ch. 5 - A 50-mL solution of a dilute AgNO3 solution is...Ch. 5 - A 0.470-g sample of magnesium reacts with 200 g...Ch. 5 - Dissolving 6.00 g CaCl2 in 300 mL of water causes...Ch. 5 - Draw an energy-level diagram (e.g., see Figure...Ch. 5 - Prob. 5.66QECh. 5 - Prob. 5.67QECh. 5 - Prob. 5.68QECh. 5 - Calculate H for the reaction...Ch. 5 - Prob. 5.70QECh. 5 - Given the thermochemical equations...Ch. 5 - In the process of isolating iron from its ores,...Ch. 5 - Prob. 5.73QECh. 5 - Prob. 5.75QECh. 5 - Prob. 5.77QECh. 5 - Prob. 5.78QECh. 5 - Prob. 5.79QECh. 5 - Prob. 5.80QECh. 5 - Prob. 5.81QECh. 5 - Prob. 5.82QECh. 5 - Calculate H when a 38-g sample of glucose,...Ch. 5 - Prob. 5.84QECh. 5 - The octane number of gasoline is based on a...Ch. 5 - One of the components of jet engine fuel is...Ch. 5 - Prob. 5.87QECh. 5 - Prob. 5.88QECh. 5 - When a 2.30-g sample of magnesium dissolves in...Ch. 5 - Prob. 5.90QECh. 5 - Prob. 5.91QECh. 5 - What mass of acetylene, C2H2(g), must be burned to...Ch. 5 - It takes 677 J of heat to increase the temperature...Ch. 5 - Prob. 5.94QECh. 5 - Prob. 5.96QECh. 5 - The enthalpy of combustion of liquid n-hexane,...Ch. 5 - What is Hrxn for reaction of iron(III) oxide and...Ch. 5 - Prob. 5.99QECh. 5 - Prob. 5.100QECh. 5 - In the 1880s, Frederick Trouton noted that the...Ch. 5 - Prob. 5.102QECh. 5 - Prob. 5.103QECh. 5 - Prob. 5.104QECh. 5 - Prob. 5.105QECh. 5 - A compound is 82.7% carbon and 17.3% hydrogen, and...Ch. 5 - Prob. 5.107QECh. 5 - Prob. 5.108QE
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
- A 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form MgCl2(aq) and H2(g). The temperature increases by 10.9 C as the magnesium reacts. Assume that the mixture has the same specific heat as water and a mass of 200 g. (a) Calculate the enthalpy change for the reaction. Is the process exothermic or endothermic? (b) Write the chemical equation and evaluate H.arrow_forwardThe enthalpy change for the following reaction is 393.5 kJ. C(s,graphite)+O2(g)CO2(g) (a) Is energy released from or absorbed by the system in this reaction? (b) What quantities of reactants and products are assumed? (c) Predict the enthalpy change observed when 3.00 g carbon burns in an excess of oxygen.arrow_forwardCompounds with carboncarbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation. C2H4(g)+H2(g)C2H6(g) Calculate the enthalpy change for this reaction, using the following combustion data: C2H4(g)+3O2(g)2CO2(g)+2H2O(l);H=1411kJC2H6(g)+72O2(g)2CO2(g)+3H2O(l);H=1560kJH2(g)+12O2(g)H2O(l);H=286kJarrow_forward
- Assume 200. mL of 0.400 M HCl is mixed with 200. mL of 0.400 M NaOH in a coffee-cup calorimeter The temperature of the solutions before mixing was 25.10 C; after mixing and allowing the reaction to occur, the temperature is 27.78 C. What is the enthalpy change when one mole of acid is neutralized? (Assume that the densities of all solutions are 1.00 g/mL and their specific heat capacities are 4.20 J/g K.)arrow_forwardWhat mass of acetylene, C2H2(g), must be burned to produce 3420 kJ of heat, given that its enthalpy of combustion is 1301 kJ/mol? Compare this with the answer to Exercise 5.91 and determine which substance produces more heat per gram.arrow_forwardThe first step in the preparation of lead from its ore (galena, PbS) consists of roasting the ore. PbS(s)+32O2(g)SO2(g)+PbO(s) Calculate the standard enthalpy change for this reaction, using enthalpies of formation (see Appendix C).arrow_forward
- When 2.50 g of methane burns in oxygen, 125 kJ of heat is produced. What is the enthalpy of combustion per mole of methane under these conditions?arrow_forwardThe Romans used calcium oxide, CaO, to produce a strong mortar to build stone structures. Calcium oxide was mixed with water to give Ca(OH)2, which reacted slowly with CO2 in the air to give CaCO3. Ca(OH)2(s) + CO2(g) CaCO3(s) + H2O(g) (a) Calculate the standard enthalpy change for this reaction. (b) How much energy is evolved or absorbed as heat if 1.00 kg of Ca(OH)2 reacts with a stoichiometric amount of CO2?arrow_forwardUsing the data in Appendix G, calculate the standard enthalpy change for each of the following reactions: (a) Si(s)+2F2(g)SiF4(g) (b) 2C(s)+2H2(g)+O2(g)CH3CO2H(l) (c) CH4(g)+N2(g)HCN(g)+NH3(g) ; (d) CS2(g)+3Cl2(g)CCl4(g)+S2Cl2(g)arrow_forward
- The thermochemical equation for the burning of methane, the main component of natural gas, is CH4(g)+2O2(g)CO2(g)+2H2O(l)H=890kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = 890 kJ? (c) What is the enthalpy change when 1.00 g methane burns in an excess of oxygen?arrow_forwardThe combustion of 1.00 mol liquid methyl alcohol (CH3OH) in excess oxygen is exothermic, giving 727 kJ of heat. (a) Write the thermochemical equation for this reaction. (b) Calculate the enthalpy change that accompanies the burning 10.0 g methanol. (c) Compare this with the amount of heat produced by 10.0 g octane, C8H18, a component of gasoline (see Exercise 5.41).arrow_forwardUse Hesss law to calculate the enthalpy change for the formation of CS2() from C(s) and S(s) [C(s) + 2 S(s) CS2()] from the following enthalpy values. C(s)+O2(g)CO2(g)rH1=393.5kJ/mol-rxnS(s)+O2(g)SO2(g)rH2=296.8kJ/mol-rxnCS2(l)+3O2(g)CO2(g)+2SO2(g)rH3=1103.9kJ/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 LearningGeneral 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 LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry 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
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
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
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