Chemistry with Access Code, Hybrid Edition
9th Edition
ISBN: 9781285188492
Author: Steven S. Zumdahl
Publisher: CENGAGE L
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 17, Problem 8ALQ
Is ∆Ssurr favorable or unfavorable for exothermic reactions? Endothermic reactions? Explain.
Expert Solution & Answer
Trending nowThis is a popular solution!
Chapter 17 Solutions
Chemistry with Access Code, Hybrid Edition
Ch. 17 - Define the following: a. spontaneous process b....Ch. 17 - What is the second law of thermodynamics? For any...Ch. 17 - What determines Ssurr for a process? To calculate...Ch. 17 - The free energy change, G, for a process at...Ch. 17 - What is the third law of thermodynamics? What are...Ch. 17 - What is the standard free energy change, G, for a...Ch. 17 - If you calculate a value for G for a reaction...Ch. 17 - Consider the equation G = G + RT ln(Q). What is...Ch. 17 - Even if G is negative, the reaction may not occur....Ch. 17 - Discuss the relationship between wmax and the...
Ch. 17 - For the process A(l) A(g), which direction is...Ch. 17 - For a liquid, which would you expect to be larger,...Ch. 17 - Gas A2 reacts with gas B2 to form gas AB at a...Ch. 17 - What types of experiments can be carried out to...Ch. 17 - A friend tells you, Free energy G and pressure P...Ch. 17 - Prob. 6ALQCh. 17 - Predict the sign of S for each of the following...Ch. 17 - Is Ssurr favorable or unfavorable for exothermic...Ch. 17 - At 1 atm, liquid water is heated above 100C. For...Ch. 17 - When (if ever) are high temperatures unfavorable...Ch. 17 - The synthesis of glucose directly from CO2 and H2O...Ch. 17 - When the environment is contaminated by a toxic or...Ch. 17 - Entropy has been described as times arrow....Ch. 17 - Human DNA contains almost twice as much...Ch. 17 - A mixture of hydrogen gas and chlorine gas remains...Ch. 17 - Consider the following potential energy plots: a....Ch. 17 - Ssurr is sometimes called the energy disorder...Ch. 17 - Given the following illustration, what can be said...Ch. 17 - The third law of thermodynamics states that the...Ch. 17 - The deciding factor on why HF is a weak acid and...Ch. 17 - List three different ways to calculate the...Ch. 17 - What information can be determined from G for a...Ch. 17 - Monochloroethane (C2H5Cl) can be produced by the...Ch. 17 - At 1500 K, the process I2(g)2I(g)10atm10atm is not...Ch. 17 - Which of the following processes are spontaneous?...Ch. 17 - Which of the following processes are spontaneous?...Ch. 17 - Table 16-1 shows the possible arrangements of four...Ch. 17 - Consider the following illustration of six...Ch. 17 - Consider the following energy levels, each capable...Ch. 17 - Redo Exercise 29 with two particles A and B, which...Ch. 17 - Choose the substance with the larger positional...Ch. 17 - Which of the following involve an increase in the...Ch. 17 - Predict the sign of Ssurr for the following...Ch. 17 - Calculate Ssurr for the following reactions at 25C...Ch. 17 - Given the values of H and S, which of the...Ch. 17 - At what temperatures will the following processes...Ch. 17 - Ethanethiol (C2H5SH; also called ethyl mercaptan)...Ch. 17 - For mercury, the enthalpy of vaporization is 58.51...Ch. 17 - For ammonia (NH3), the enthalpy of fusion is 5.65...Ch. 17 - The enthalpy of vaporization of ethanol is 38.7...Ch. 17 - Predict the sign of S for each of the following...Ch. 17 - Predict the sign of S for each of the following...Ch. 17 - For each of the following pairs of substances,...Ch. 17 - For each of the following pairs, which substance...Ch. 17 - Predict the sign of S and then calculate S for...Ch. 17 - Predict the sign of S and then calculate S for...Ch. 17 - For the reaction C2H2(g)+4F2(g)2CF4(g)+H2(g) S is...Ch. 17 - For the reaction CS2(g)+3O2(g)CO2(g)+2SO2(g) S is...Ch. 17 - It is quite common for a solid to change from one...Ch. 17 - Two crystalline forms of white phosphorus are...Ch. 17 - Consider the reaction 2O(g)O2(g) a. Predict the...Ch. 17 - Hydrogen cyanide is produced industrially by the...Ch. 17 - From data in Appendix 4, calculate H, S, and G for...Ch. 17 - The major industrial use of hydrogen is in the...Ch. 17 - For the reaction at 298 K, 2NO2(g)N2O4(g) the...Ch. 17 - At 100C and 1.00 atm, H = 40.6 kJ/mol for the...Ch. 17 - Given the following data:...Ch. 17 - Given the following data:...Ch. 17 - For the reaction SF4(g)+F2(g)SF6(g) the value of G...Ch. 17 - The value of G for the reaction...Ch. 17 - Consider the reaction...Ch. 17 - Consider the reaction 2POCl3(g)2PCl3(g)+O2(g) a....Ch. 17 - Using data from Appendix 4, calculate H, S and G...Ch. 17 - Consider two reactions for the production of...Ch. 17 - Using data from Appendix 4, calculate G for the...Ch. 17 - Using data from Appendix 4, calculate G for the...Ch. 17 - Consider the reaction 2NO2(g)N2O4(g) For each of...Ch. 17 - Consider the following reaction:...Ch. 17 - One of the reactions that destroys ozone in the...Ch. 17 - Hydrogen sulfide can be removed from natural gas...Ch. 17 - Consider the following reaction at 25.0C:...Ch. 17 - The standard free energies of formation and the...Ch. 17 - Calculate G forH2O(g)+12O2(g)H2O2(g) at 600. K,...Ch. 17 - The Ostwald process for the commercial production...Ch. 17 - Cells use the hydrolysis of adenosine...Ch. 17 - One reaction that occurs in human metabolism is...Ch. 17 - Consider the following reaction at 800. K:...Ch. 17 - Consider the following reaction at 298 K:...Ch. 17 - Consider the relationship In(K)=HRT+SR The...Ch. 17 - The equilibrium constant K for the reaction...Ch. 17 - Using Appendix 4 and the following data, determine...Ch. 17 - Some water is placed in a coffee-cup calorimeter....Ch. 17 - Calculate the entropy change for the vaporization...Ch. 17 - As O2(l) is cooled at 1 atm, it freezes at 54.5 K...Ch. 17 - Consider the following reaction:...Ch. 17 - Using the following data, calculate the value of...Ch. 17 - Many biochemical reactions that occur in cells...Ch. 17 - Carbon monoxide is toxic because it bonds much...Ch. 17 - In the text, the equation G=G+RTIn(Q) was derived...Ch. 17 - Prob. 91AECh. 17 - Use the equation in Exercise 79 to determine H and...Ch. 17 - Prob. 93AECh. 17 - Consider the following diagram of free energy (G)...Ch. 17 - Prob. 95CWPCh. 17 - For rubidium Hvapo=69.0KJ/mol at 686C, its boiling...Ch. 17 - Given the thermodynamic data below, calculate S...Ch. 17 - Consider the reaction: H2S(g)+SO2(g)3S(g)+2H2O(l)...Ch. 17 - The following reaction occurs in pure water:...Ch. 17 - Prob. 100CWPCh. 17 - Consider the reaction: PCl3(g)+Cl2(g)PCl5(g) At...Ch. 17 - The equilibrium constant for a certain reaction...Ch. 17 - Consider two perfectly insulated vessels. Vessel 1...Ch. 17 - Liquid water at 25C is introduced into an...Ch. 17 - Using data from Appendix 4, calculate H, G, and K...Ch. 17 - Entropy can be calculated by a relationship...Ch. 17 - a. Using the free energy profile for a simple...Ch. 17 - Consider the reaction H2(g)+Br2(g)2HBr(g) where H...Ch. 17 - Consider the system A(g)B(g) at25C. a. Assuming...Ch. 17 - The equilibrium constant for a certain reaction...Ch. 17 - If wet silver carbonate is dried in a stream of...Ch. 17 - Carbon tetrachloride (CCl4) and benzene (C6H6)...Ch. 17 - Sodium chloride is added to water (at 25C) until...Ch. 17 - You have a 1.00-L sample of hot water (90.0C)...Ch. 17 - Consider a weak acid, HX. If a 0.10-M solution of...Ch. 17 - Some nonelectrolyte solute (molar mass = 142...Ch. 17 - For the equilibrium A(g)+2B(g)C(g) the initial...Ch. 17 - What is the pH of a 0. 125-M solution of the weak...Ch. 17 - Impure nickel, refined by smelting sulfide ores in...
Additional Science Textbook Solutions
Find more solutions based on key concepts
6. How can you use the features found in each chapter?
Human Anatomy & Physiology (2nd Edition)
What were the major microbiological interests of Martinus Beijerinck and Sergei Winogradsky? It can be said tha...
Brock Biology of Microorganisms (15th Edition)
Give the IUPAC name for each compound.
Organic Chemistry
45. Calculate the mass of nitrogen dissolved at room temperature in an 80.0-L home aquarium. Assume a total pre...
Chemistry: Structure and Properties (2nd Edition)
How could you separate a mixture of the following compounds? The reagents available to you are water, either, 1...
Organic Chemistry (8th Edition)
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
- Thermodynamics provides a way to interpret everyday occurrences. If you live in northern climates, one common experience is that during early winter, snow falls but then melts when it hits the ground. Both the formation and the melting happen spontaneously. How can thermodynamics explain both of these seemingly opposed events?arrow_forwardThe equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (H) for this reaction (assuming H is temperature-independent).arrow_forwardFor the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)arrow_forward
- The decomposition of diamond to graphite [C(diamond) C(graphite)] is thermodynamically favored, but occurs slowly at room temperature. a. Use fG values from Appendix L to calculate rG and Keq for the reaction under standard conditions and 298.15 K. b. Use fH and S values from Appendix L to estimate rG and Keq for the reaction at 1000 K. Assume that enthalpy and entropy values are valid at these temperatures. Does heating shift the equilibrium toward the formation of diamond or graphite? c. Why is the formation of diamond favored at high pressures? d. The phase diagram shows that diamond is thermodynamically favored over graphite at 20,000 atmospheres pressure (about 2 GPa) at room temperature. Why is this conversion actually done at much higher temperatures and pressures?arrow_forward9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of 0.50 M NaOH in a coffee cup calorimeter. Both solutions were initially at 20.0°C, but when the two were mixed, the temperature rose to 23.2°C. (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why?arrow_forwardWhen 7.11 g NH4NO3 is added to 100 mL water, the temperature of the calorimeter contents decreases from 22.1 C to 17.1 C. Assuming that the mixture has the same specific heat as water and a mass of 107 g, calculate the heat q. Is the dissolution of ammonium nitrate exothermic or endothermic?arrow_forward
- For the reaction TiCl2(s) + Cl2(g) TiCl4(), rG = 272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of fG for TiCl2(s).arrow_forwardCoal is used as a fuel in some electric-generating plants. Coal is a complex material, but for simplicity we may consider it to be a form of carbon. The energy that can be derived from a fuel is sometimes compared with the enthalpy of the combustion reaction: C(s)+O2(g)CO2(g) Calculate the standard enthalpy change for this reaction at 25C. Actually, only a fraction of the heat from this reaction is available to produce electric energy. In electric generating plants, this reaction is used to generate heat for a steam engine, which turns the generator. Basically the steam engine is a type of heat engine in which steam enters the engine at high temperature (Th), work is done, and the steam then exits at a lower temperature (Tl). The maximum fraction, f, of heat available to produce useful energy depends on the difference between these temperatures (expressed in kelvins), f = (Th Tl)/Th. What is the maximum heat energy available for useful work from the combustion of 1.00 mol of C(s) to CO2(g)? (Assume the value of H calculated at 25C for the heat obtained in the generator.) It is possible to consider more efficient ways to obtain useful energy from a fuel. For example, methane can be burned in a fuel cell to generate electricity directly. The maximum useful energy obtained in these cases is the maximum work, which equals the free-energy change. Calculate the standard free-energy change for the combustion of 1.00 mol of C(s) to CO2(g). Compare this value with the maximum obtained with the heat engine described here.arrow_forwardWhat is meant by the standard free-energy change G for a reaction? What is meant by the standard free energy of formation Gf of a substance?arrow_forward
- Define the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universearrow_forwardUsing values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2 H2O() 2 NaOH(aq) + H2(g) (b) 6 C(graphite) + 3 H2(g) C6H6() Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?arrow_forwardIs the formation of ozone (O3(g)) from oxygen (O2(g)) spontaneous at room temperature under standard state conditions?arrow_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 Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
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