Chemistry: An Atoms First Approach
2nd Edition
ISBN: 9781305079243
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
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Chapter 16, Problem 116CP
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Chapter 16 Solutions
Chemistry: An Atoms First Approach
Ch. 16 - Define the following: a. spontaneous process b....Ch. 16 - What is the second law of thermodynamics? For any...Ch. 16 - Prob. 3RQCh. 16 - Prob. 4RQCh. 16 - Prob. 5RQCh. 16 - What is the standard free energy change, G, for a...Ch. 16 - If you calculate a value for G for a reaction...Ch. 16 - Consider the equation G = G + RT ln(Q). What is...Ch. 16 - Even if G is negative, the reaction may not occur....Ch. 16 - Prob. 10RQ
Ch. 16 - For the process A(l) A(g), which direction is...Ch. 16 - Prob. 2ALQCh. 16 - Gas A2 reacts with gas B2 to form gas AB at a...Ch. 16 - Prob. 4ALQCh. 16 - Prob. 5ALQCh. 16 - Prob. 6ALQCh. 16 - Predict the sign of S for each of the following...Ch. 16 - Is Ssurr favorable or unfavorable for exothermic...Ch. 16 - At 1 atm, liquid water is heated above 100C. For...Ch. 16 - Prob. 10ALQCh. 16 - The synthesis of glucose directly from CO2 and H2O...Ch. 16 - When the environment is contaminated by a toxic or...Ch. 16 - Entropy has been described as times arrow....Ch. 16 - Prob. 14QCh. 16 - A mixture of hydrogen gas and chlorine gas remains...Ch. 16 - Consider the following potential energy plots: a....Ch. 16 - Prob. 17QCh. 16 - Given the following illustration, what can be said...Ch. 16 - The third law of thermodynamics states that the...Ch. 16 - Prob. 20QCh. 16 - Prob. 21QCh. 16 - Prob. 22QCh. 16 - Monochloroethane (C2H5Cl) can be produced by the...Ch. 16 - Prob. 24QCh. 16 - Which of the following processes are spontaneous?...Ch. 16 - Which of the following processes are spontaneous?...Ch. 16 - Prob. 27ECh. 16 - Consider the following illustration of six...Ch. 16 - Consider the following energy levels, each capable...Ch. 16 - Prob. 30ECh. 16 - Choose the substance with the larger positional...Ch. 16 - Which of the following involve an increase in the...Ch. 16 - Predict the sign of Ssurr for the following...Ch. 16 - Prob. 34ECh. 16 - Given the values of H and S, which of the...Ch. 16 - At what temperatures will the following processes...Ch. 16 - Ethanethiol (C2H5SH; also called ethyl mercaptan)...Ch. 16 - For mercury, the enthalpy of vaporization is 58.51...Ch. 16 - For ammonia (NH3), the enthalpy of fusion is 5.65...Ch. 16 - The enthalpy of vaporization of ethanol is 38.7...Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Prob. 42ECh. 16 - Prob. 43ECh. 16 - For each of the following pairs, which substance...Ch. 16 - Predict the sign of S and then calculate S for...Ch. 16 - Predict the sign of S and then calculate S for...Ch. 16 - Prob. 47ECh. 16 - Prob. 48ECh. 16 - Prob. 49ECh. 16 - Two crystalline forms of white phosphorus are...Ch. 16 - Consider the reaction 2O(g)O2(g) a. Predict the...Ch. 16 - Prob. 52ECh. 16 - Prob. 53ECh. 16 - The major industrial use of hydrogen is in the...Ch. 16 - Prob. 55ECh. 16 - At 100C and 1.00 atm, H = 40.6 kJ/mol for the...Ch. 16 - Prob. 57ECh. 16 - Prob. 58ECh. 16 - Prob. 59ECh. 16 - Prob. 60ECh. 16 - Consider the reaction...Ch. 16 - Consider the reaction 2POCl3(g)2PCl3(g)+O2(g) a....Ch. 16 - Prob. 63ECh. 16 - Consider two reactions for the production of...Ch. 16 - Prob. 65ECh. 16 - Prob. 66ECh. 16 - Consider the reaction 2NO2(g)N2O4(g) For each of...Ch. 16 - Prob. 68ECh. 16 - One of the reactions that destroys ozone in the...Ch. 16 - Hydrogen sulfide can be removed from natural gas...Ch. 16 - Consider the following reaction at 25.0C:...Ch. 16 - The standard free energies of formation and the...Ch. 16 - Calculate G forH2O(g)+12O2(g)H2O2(g) at 600. K,...Ch. 16 - The Ostwald process for the commercial production...Ch. 16 - Cells use the hydrolysis of adenosine...Ch. 16 - One reaction that occurs in human metabolism is...Ch. 16 - Prob. 77ECh. 16 - Consider the following reaction at 298 K:...Ch. 16 - Prob. 79ECh. 16 - The equilibrium constant K for the reaction...Ch. 16 - Prob. 81AECh. 16 - Some water is placed in a coffee-cup calorimeter....Ch. 16 - Consider the following system at equilibrium at...Ch. 16 - Calculate the entropy change for the vaporization...Ch. 16 - As O2(l) is cooled at 1 atm, it freezes at 54.5 K...Ch. 16 - Prob. 86AECh. 16 - Using the following data, calculate the value of...Ch. 16 - Prob. 88AECh. 16 - Carbon monoxide is toxic because it bonds much...Ch. 16 - Prob. 90AECh. 16 - Prob. 91AECh. 16 - Use the equation in Exercise 79 to determine H and...Ch. 16 - Consider the reaction...Ch. 16 - Consider the following diagram of free energy (G)...Ch. 16 - Prob. 95CWPCh. 16 - For rubidium Hvapo=69.0KJ/mol at 686C, its boiling...Ch. 16 - Given the thermodynamic data below, calculate S...Ch. 16 - Prob. 98CWPCh. 16 - Prob. 99CWPCh. 16 - Consider the dissociation of a weak acid HA (Ka =...Ch. 16 - Prob. 101CWPCh. 16 - The equilibrium constant for a certain reaction...Ch. 16 - For the following reactions at constant pressure,...Ch. 16 - The standard enthalpy of formation of H2O(l) at...Ch. 16 - Prob. 105CPCh. 16 - Liquid water at 25C is introduced into an...Ch. 16 - Using data from Appendix 4, calculate H, G, and K...Ch. 16 - Prob. 108CPCh. 16 - Prob. 109CPCh. 16 - Prob. 110CPCh. 16 - Prob. 111CPCh. 16 - Prob. 112CPCh. 16 - If wet silver carbonate is dried in a stream of...Ch. 16 - Carbon tetrachloride (CCl4) and benzene (C6H6)...Ch. 16 - Sodium chloride is added to water (at 25C) until...Ch. 16 - Prob. 116CPCh. 16 - Prob. 117CPCh. 16 - Prob. 118IPCh. 16 - Prob. 119IPCh. 16 - Prob. 120IPCh. 16 - Consider a sample containing 5.00 moles of a...Ch. 16 - Impure nickel, refined by smelting sulfide ores in...
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- 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 decomposition of ozone, O3, to oxygen, O2, is an exothermic reaction. What is the sign of q? If you were to touch a flask in which ozone is decomposing to oxygen, would you expect the flask to feel warm or cool?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_forward
- A green plant synthesizes glucose by photosynthesis, as shown in the reaction: 6CO2(g) + 6H2O(l) C6H12O6(s) + 6O2(g) Animals use glucose as a source of energy: C6H12O6(s) + 6O2(g) 6CO2(g) + 6HO2(l) If we were to assume that both of these processes occur to the same extent in a cyclic process, what thermodynamic property must have a nonzero value?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_forwardAthletic trainers use instant ice packs that can be cooled quickly on demand. Squeezing the pact breaks an inner container, allowing two components to mix and react. This reaction makes the pack become cold. Describe the heat flow for this spontaneous process.arrow_forward
- What is entropy? Why is entropy important?arrow_forwardHow is the sign of q, heat, defined? How does it relate to the total energy of the system?arrow_forwardOne statement of the second law of thermodynamics is that heat cannot be turned completely into work. Another is that the entropy of the universe always increases. How are these two statements related?arrow_forward
- Two crystalline forms of white phosphorus are known. Both forms contain P4 molecules, but the molecules are packed together in different ways. The form is always obtained when the liquid freezes. However, below 76.9C, the form spontaneously converts to the form: P4(s,)P4(s,) a. Predict the signs of H and S for this process. b. Predict which form of phosphorus has the more ordered crystalline structure (has the smaller positional probability).arrow_forward9.20 State the first law of thermodynamics briefly in your own words.arrow_forwardFor each process, tell whether the entropy change of the system is positive or negative. Water vapor (the system) deposits as ice crystals on a cold windowpane. A can of carbonated beverage loses its fizz. (Consider the beverage but not the can as the system. What happens to the entropy of the dissolved gas?) A glassblower heats glass (the system) to its softening temperature.arrow_forward
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