General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 16.6, Problem 16.6P
By determining the sign of ΔStotal, show whether the decomposition of calcium carbonate is spontaneous under standard-state conditions at 25 °C.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 16 Solutions
General Chemistry: Atoms First
Ch. 16.1 - Predicting the Sign of S Predict the sign of S in...Ch. 16.2 - Prob. 16.2PCh. 16.2 - Prob. 16.3CPCh. 16.3 - Which state has the higher entropy? Explain in...Ch. 16.5 - Calculate the standard entropy of reaction at 25C...Ch. 16.6 - By determining the sign of Stotal, show whether...Ch. 16.7 - Consider the decomposition of gaseous N2O4:...Ch. 16.7 - The following data apply to the vaporization of...Ch. 16.7 - What are the signs (+, , or 0) of H, S, and G for...Ch. 16.8 - Consider the thermal decomposition of calcium...
Ch. 16.8 - Consider the following endothermic decomposition...Ch. 16.9 - (a)Using values of Gf in Appendix B, calculate the...Ch. 16.10 - Calculate G for the formation of ethylene (C2H4)...Ch. 16.10 - Consider the following gas-phase reaction of A2...Ch. 16.11 - Given the data in Appendix B, calculate Kp at 25 C...Ch. 16.11 - Use the data in Appendix B to calculate the vapor...Ch. 16.11 - At 25 C, Kw for the dissociation of water is 1.0 ...Ch. 16.11 - Prob. 16.18PCh. 16.11 - Prob. 16.19PCh. 16 - Ideal gases A (red spheres) and B (blue spheres)...Ch. 16 - What are the signs (+, , or 0) of H, S, and G for...Ch. 16 - What are the signs (+, , or 0) of H, S, and G for...Ch. 16 - An ideal gas is compressed at constant...Ch. 16 - Consider the following spontaneous reaction of A2...Ch. 16 - Consider the dissociation reactionA2(g)2A(g). The...Ch. 16 - Prob. 16.26CPCh. 16 - Prob. 16.27CPCh. 16 - Prob. 16.28CPCh. 16 - Prob. 16.29CPCh. 16 - Prob. 16.30SPCh. 16 - Prob. 16.31SPCh. 16 - Prob. 16.32SPCh. 16 - Prob. 16.33SPCh. 16 - Prob. 16.34SPCh. 16 - Prob. 16.35SPCh. 16 - Prob. 16.36SPCh. 16 - Prob. 16.37SPCh. 16 - Prob. 16.38SPCh. 16 - Predict the sign of S for each process in Problem...Ch. 16 - Prob. 16.40SPCh. 16 - Prob. 16.41SPCh. 16 - Prob. 16.42SPCh. 16 - Prob. 16.43SPCh. 16 - Prob. 16.44SPCh. 16 - Prob. 16.45SPCh. 16 - Which state in each of the following pairs has the...Ch. 16 - Which State in each of the following pairs has the...Ch. 16 - Prob. 16.48SPCh. 16 - Prob. 16.49SPCh. 16 - Prob. 16.50SPCh. 16 - Which substance in each of the following pairs...Ch. 16 - Prob. 16.52SPCh. 16 - Prob. 16.53SPCh. 16 - Prob. 16.54SPCh. 16 - Prob. 16.55SPCh. 16 - Prob. 16.56SPCh. 16 - Prob. 16.57SPCh. 16 - Prob. 16.58SPCh. 16 - Prob. 16.59SPCh. 16 - Prob. 16.60SPCh. 16 - Prob. 16.61SPCh. 16 - In lightning storms, oxygen is converted to ozone:...Ch. 16 - Sulfur dioxide emitted from coal-fired power...Ch. 16 - Elemental mercury can be produced from its oxide:...Ch. 16 - Prob. 16.65SPCh. 16 - For the vaporization of benzene, Hvap = 30.7kJ/mol...Ch. 16 - For the melting of sodium chloride, Hfusion =...Ch. 16 - Prob. 16.68SPCh. 16 - Prob. 16.69SPCh. 16 - Prob. 16.70SPCh. 16 - Prob. 16.71SPCh. 16 - Prob. 16.72SPCh. 16 - Given the data in Problem 16.67, calculate G for...Ch. 16 - Prob. 16.74SPCh. 16 - Prob. 16.75SPCh. 16 - Prob. 16.76SPCh. 16 - Prob. 16.77SPCh. 16 - Prob. 16.78SPCh. 16 - Use the data in Appendix B to calculate H and S...Ch. 16 - Prob. 16.80SPCh. 16 - Prob. 16.81SPCh. 16 - Use the data in Appendix B to tell which of the...Ch. 16 - Prob. 16.83SPCh. 16 - Prob. 16.84SPCh. 16 - Prob. 16.85SPCh. 16 - Ethanol is manufactured in industry by the...Ch. 16 - Sulfur dioxide in the effluent gases from...Ch. 16 - Prob. 16.88SPCh. 16 - Prob. 16.89SPCh. 16 - Prob. 16.90SPCh. 16 - Prob. 16.91SPCh. 16 - Prob. 16.92SPCh. 16 - What is G for the formation of solid uranium...Ch. 16 - Prob. 16.94SPCh. 16 - Prob. 16.95SPCh. 16 - What is the relationship between the standard...Ch. 16 - What is the relationship between the standard...Ch. 16 - Prob. 16.98SPCh. 16 - Prob. 16.99SPCh. 16 - Prob. 16.100SPCh. 16 - At 25 C, Ka for acid dissociation of aspirin...Ch. 16 - Prob. 16.102SPCh. 16 - Calculate the equilibrium partial pressure of...Ch. 16 - Ethylene oxide, C2H4O, is used to make antifreeze...Ch. 16 - The first step in the commercial production of...Ch. 16 - Prob. 16.106CHPCh. 16 - Prob. 16.107CHPCh. 16 - Prob. 16.108CHPCh. 16 - Prob. 16.109CHPCh. 16 - Prob. 16.110CHPCh. 16 - The standard free-energy change at 25 C for the...Ch. 16 - Prob. 16.112CHPCh. 16 - Prob. 16.113CHPCh. 16 - Prob. 16.114CHPCh. 16 - Prob. 16.115CHPCh. 16 - Use the data in Appendix B to calculate H, S, and...Ch. 16 - Troutons rule says that the ratio of the molar...Ch. 16 - Prob. 16.118CHPCh. 16 - Prob. 16.119CHPCh. 16 - Prob. 16.120CHPCh. 16 - Use the data in Appendix B to calculate the...Ch. 16 - Prob. 16.122CHPCh. 16 - Prob. 16.123CHPCh. 16 - Prob. 16.124CHPCh. 16 - Prob. 16.125CHPCh. 16 - Prob. 16.126CHPCh. 16 - Prob. 16.127CHPCh. 16 - Prob. 16.128CHPCh. 16 - Prob. 16.129CHPCh. 16 - Prob. 16.130CHPCh. 16 - Prob. 16.131CHPCh. 16 - Prob. 16.132CHPCh. 16 - Prob. 16.133MPCh. 16 - Prob. 16.134MPCh. 16 - One step in the commercial synthesis of sulfuric...Ch. 16 - Prob. 16.136MPCh. 16 - Prob. 16.137MPCh. 16 - A 1.00 L volume of gaseous ammonia at 25.0 C and...Ch. 16 - Consider the unbalanced equation:...Ch. 16 - A mixture of NO2 and N2O4, each at an initial...
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
- Define the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universearrow_forwardIndicate whether the following processes are spontaneous or nonspontaneous. (a) Liquid water freezing at a temperature below its freezing point (b) Liquid water freezing at a temperature above its freezing point (c) The combustion of gasoline (d) A ball thrown into the air (e) A raindrop falling to the ground (f) Iron rusting in a moist atmospherearrow_forwardFor each process, predict whether entropy increases or decreases, and explain how you arrived at your prediction. 2 CO2(g) → 2 CO(g) + O2(g) NaCl(s) → NaCl(aq) MgCO3(s) → MgO(s) + CO2(g)arrow_forward
- Use the data in Appendix G to calculate the standard entropy change for H2(g) + CuO(s) H2O() + Cu(s)arrow_forwardChemists and engineers who design nuclear power plants have to worry about high-temperature reactions because it is possible for water to decompose. (a) Under what conditions does this reaction occur spontaneously? 2H2O(g) 2H2(g) + O2(g) (b) Under conditions where the decomposition of water is spontaneous, do nuclear engineers have to worry about an oxygen/hydrogen explosion? Justify your answer.arrow_forwardConsider the reaction of 2 mol H2(g) at 25C and 1 atm with 1 mol O2(g) at the same temperature and pressure to produce liquid water at these conditions. If this reaction is run in a controlled way to generate work, what is the maximum useful work that can be obtained? How much entropy is produced in this case?arrow_forward
- Sodium reacts violently with water according to the equation Na(s) + H2O() NaOH(aq) + H2(g) Without doing calculations, predict the signs of rH and rS for the reaction. Verify your prediction with a calculation.arrow_forwardThere are millions of organic compounds known, and new ones are being discovered or made at a rate of morethan 100,000 compounds per year. Organic compoundsburn readily in air at high temperatures to form carbondioxide and water. Several classes of organic compoundsare listed, with a simple example of each. Write a balanced chemical equation for the combustion in O2ofeach of these compounds, and then use the data inAppendix J to show that each reaction is product-favoredat room temperature. From these results, it is reasonable to hypothesize thatallorganic compounds are thermodynamically unstable inan oxygen atmosphere (that is, their room-temperaturereaction with O2(g) to form CO2(g) and H2O() isproduct-favored). If this hypothesis is true, how canorganic compounds exist on Earth?arrow_forwardThe combustion of acetylene, C2H2, is a spontaneous reaction given by the equation 2C2H2(g)+5O2(g)4CO2(g)+2H2O(l) As expected for a combustion, the reaction is exothermic. What is the sign of H? What do you expect for the sign of S? Explain the spontaneity of the reaction in terms of the enthalpy and entropy changes.arrow_forward
- Silver carbonate, Ag2CO3, is a light yellow compound that decomposes when heated to give silver oxide and carbon dioxide: Ag2CO3(s)Ag2O(s)+CO2(g) A researcher measured the partial pressure of carbon dioxide over a sample of silver carbonate at 220C and found that it was 1.37 atm. Calculate the partial pressure of carbon dioxide at 25C. The standard enthalpies of formation of silver carbonate and silver oxide at 25C are 505.9 kJ/mol and 31.05 kJ/mol, respectively. Make any reasonable assumptions in your calculations. State the assumptions that you make, and note why you think they are reasonable.arrow_forwardThe molecular scale pictures below show snapshots of a strong acid at three different instants after it is added to water. Place the three pictures in the correct order so that they show the progress of the spontaneous process that takes place as the acid dissolves in the water. Explain your answer in terms of entropyarrow_forwardYeast can produce ethanol by the fermentation of glucose (C6H12O6), which is the basis for the production of most alcoholic beverages. C6H12O6(aq) 2 C2H5OH() + 2 CO2(g) Calculate rH, rS, and rG for the reaction at 25 C. Is the reaction product- or reactant-favored at equilibrium? In addition to the thermodynamic values in Appendix L, you will need the following data for C6H12O6(aq): fH = 1260.0 kl/mol; S = 289 J/K mol; and fG = 918.8 kl/mol.arrow_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 by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher: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 by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
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
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