Chemistry for Engineering Students
4th Edition
ISBN: 9781337398909
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 10, Problem 10.16PAE
Murphy's law is a whimsical rule that says that anything that can go wrong will go wrong. But in an article in the Journal of Chemical Education, Frank Lambert writes, "Murphy's law is a fraud." He also writes, "The second law of
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Chapter 10 Solutions
Chemistry for Engineering Students
Ch. 10 - Prob. 1COCh. 10 - . explain the concept of entropy in your own...Ch. 10 - Prob. 3COCh. 10 - . state the second law of thermodynamics in words...Ch. 10 - Prob. 5COCh. 10 - Prob. 6COCh. 10 - Prob. 7COCh. 10 - Prob. 8COCh. 10 - Prob. 9COCh. 10 - Prob. 10CO
Ch. 10 - Prob. 10.1PAECh. 10 - Prob. 10.2PAECh. 10 - Prob. 10.3PAECh. 10 - Prob. 10.4PAECh. 10 - Prob. 10.5PAECh. 10 - Use the web to learn how many pounds of plastics...Ch. 10 - On the basis of your experience, predict which of...Ch. 10 - In the thermodynamic definition of a spontaneous...Ch. 10 - 1f the combustion of butane is spontaneous, how...Ch. 10 - Identify each of the processes listed as...Ch. 10 - Identify each of the processes listed as...Ch. 10 - Athletic trainers use instant ice packs that can...Ch. 10 - Are any of the following exothermic processes not...Ch. 10 - Enthalpy changes often help predict whether or not...Ch. 10 - When a fossil fuel burns, is that fossil fuel the...Ch. 10 - Murphy's law is a whimsical rule that says that...Ch. 10 - Prob. 10.17PAECh. 10 - Some games include dice with more than six sides....Ch. 10 - How does probability relate to spontaneity?Ch. 10 - Prob. 10.20PAECh. 10 - For each pair of items, tell which has the higher...Ch. 10 - For each process, tell whether the entropy change...Ch. 10 - Without doing a calculation, predict whether the...Ch. 10 - For the following chemical reactions, predict the...Ch. 10 - What happens to the entropy of the universe during...Ch. 10 - Prob. 10.26PAECh. 10 - One statement of the second law of thermodynamics...Ch. 10 - Prob. 10.28PAECh. 10 - Prob. 10.29PAECh. 10 - Which reaction occurs with the greater increase in...Ch. 10 - Which reaction occurs with the greater increase in...Ch. 10 - Methanol is burned as fuel in some race cars. This...Ch. 10 - Limestone is predominantly CaCO3, which can...Ch. 10 - Suppose that you find out that a system has an...Ch. 10 - Use tabulated thermodynamic data to calculate the...Ch. 10 - Prob. 10.36PAECh. 10 - Calculate S for the dissolution of magnesium...Ch. 10 - Calculate the standard entropy change for the...Ch. 10 - Through photosynthesis, plants build molecules of...Ch. 10 - Find websites describing two different attempts to...Ch. 10 - Prob. 10.41PAECh. 10 - Prob. 10.42PAECh. 10 - Under what conditions does G allow us to predict...Ch. 10 - There is another free energy state function, the...Ch. 10 - 10.45 Calculate G at 45°C for reactions for which...Ch. 10 - 10.46 Discuss the effect of temperature change on...Ch. 10 - The reaction CO2(g)+H2(g)CO(g)+H2O(g) is not...Ch. 10 - Prob. 10.48PAECh. 10 - Prob. 10.49PAECh. 10 - For the reaction NO(g)+NO2(g)N2O3(g) , use...Ch. 10 - 10.51 The combustion of acetylene was used in...Ch. 10 - Natural gas (methane) is being used in...Ch. 10 - Silicon forms a series of compounds analogous to...Ch. 10 - Explain why Gf of O2 (g) is zero.Ch. 10 - Using tabulated thermodynamic data, calculate G...Ch. 10 - Using tabulated thermodynamic data, calculate G...Ch. 10 - Calculate G for the dissolution of both sodium...Ch. 10 - Phosphorus exists in multiple solid phases,...Ch. 10 - 10.59 The normal melting point of benzene, C6H6,...Ch. 10 - Prob. 10.60PAECh. 10 - Estimate the temperature range over which each of...Ch. 10 - Recall that incomplete combustion of fossil fuels...Ch. 10 - During polymerization, the system usually becomes...Ch. 10 - Prob. 10.64PAECh. 10 - Prob. 10.65PAECh. 10 - The recycling of polymers represents only one...Ch. 10 - Prob. 10.67PAECh. 10 - When ice melts, its volume decreases. Despite this...Ch. 10 - 10.69 If a sample of air were separated into...Ch. 10 - Prob. 10.70PAECh. 10 - An explosion brings down an old building, leaving...Ch. 10 - Prob. 10.72PAECh. 10 - Prob. 10.73PAECh. 10 - Prob. 10.74PAECh. 10 - Prob. 10.75PAECh. 10 - Some say that the job of an engineer is to fight...Ch. 10 - A beaker of water at 40C (on the left in the...Ch. 10 - Why is it usually easier to use G to determine the...Ch. 10 - The molecular scale pictures below show snapshots...Ch. 10 - Prob. 10.80PAECh. 10 - Diethyl ether is a liquid at normal temperature...Ch. 10 - Calculate the entropy change, S , for the...Ch. 10 - Gallium metal has a melting point of 29.8°C. Use...Ch. 10 - Methane can be produced from CO and H2.The process...Ch. 10 - 10.85 Iodine is not very soluble in water, but it...Ch. 10 - The enthalpy of vaporization for water is 40.65 kJ...Ch. 10 - Determine whether each of the following statements...Ch. 10 - Nickel metal reacts with carbon monoxide to form...Ch. 10 - Polyethylene has a heat capacity of 2,3027 J g-1...Ch. 10 - A key component in many chemical engineering...Ch. 10 - The reaction shown below is involved in the...Ch. 10 - Using only the data given below, determine G for...Ch. 10 - The graph below shows G as a function of...Ch. 10 - Prob. 10.94PAECh. 10 - Prob. 10.95PAECh. 10 - Prob. 10.96PAECh. 10 - Prob. 10.97PAECh. 10 - Prob. 10.98PAECh. 10 - Thermodynamics provides a way to interpret...Ch. 10 - Prob. 10.100PAECh. 10 - 10.101 Fluorine reacts with liquid water to form...Ch. 10 - 10.102 Ammonia can react with oxygen gas to form...Ch. 10 - Prob. 10.103PAECh. 10 - 10.104 (a) When a chemical bond forms, what...
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- Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.arrow_forwardCobalt(II) chloride hexahydrate, CoCl26H2O, is a bright pink compound, but in the presence of very dry air it loses water vapor to the air to produce the light blue anhydrous salt CoCl2. Calculate the standard free-energy change for the reaction at 25C: CoCl26H2O(s)CoCl2(s)+6H2O(g) Here are some thermodynamic data at 25C: What is the partial pressure of water vapor in equilibrium with the anhydrous salt and the hexahydrate at 25C? (Give the value in mmHg.) What is the relative humidity of air that has this partial pressure of water? The relative humidity of a sample of air is Relativehumidity=partialpressureofH2O(g)inairvaporpressureofwater100 What do you expect to happen to the equilibrium partial pressure over the hexahydrate as the temperature is raised? Explain.arrow_forwardWith regard to exercise 2.50, how accurate do you think your answer is, and why?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_forwardWhat is entropy? Why is entropy important?arrow_forwardWhat is the change in entropy, S, for the reaction CaCO3(s)+2H(aq)Ca2+(aq)+H2O(l)+CO2(g) See Table 18.1 for values of standard entropies. Does the entropy of the chemical system increase or decrease as you expect? Explain.arrow_forward
- Chemical Equilibrium. a) Briefly describe why (or how) it is possible to have an absolute value for the entropy of a system. b) Write appropriate inequalities for Gibbs free energy, Entropy and the Reaction Quotient that determine the direction of spontaneous change for forward, reverse or equilibrium processes. c) Briefly describe what you expect to occur as a function of time at a “single molecule" level for the chemical reaction AB=A +B9) at equilibrium. d) For the case of c how would you determine that the system is not at equilibrium?arrow_forwardMethane and chlorine react to form chloroform and hydrogen chloride, like this: CH (g)+3Cl,(g) → CHCI3(g)+3HCI(g) The reaction is exothermic. Suppose a mixture of CH, Cl,, CHCI, and HCl has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium O to the right The temperature is lowered. O to the left The pressure of CHA will O (none) O to the right O to the left The temperature is raised. The pressure of CHCI3 will ? O (none) Check O 2021 McGraw-Hill Education, All Rights Reserved Terms of Use Pacy Explanation hparrow_forwardThe following reaction is carried out at 25.0 °C and 1.00 atm: 2NO(g) + O2(g) →→ 2NO2(g) AH0 kJmol-1 Sº JK-¹mol-1 NO (g) -110.525 197.674 NO₂ (g) -393.509 213.74 O₂ (g) 0.00 205.0 Using the data in the table: • Calculate the enthalpy of reaction, A₁H, for the reaction: mol-1 • Calculate the entropy change, ASº, for the reaction: • Calculate AGO for the reaction: kJ mol-1 Is this reaction spontaneous or not spontaneous at this temperature and pressure? kJ JK-1 mol-1arrow_forward
- Up, down or centerarrow_forwardanging... Nitrogen monoxide and water react to form ammonia and oxygen, like this: 015 Mar 4 NO(g)+6H,0(g) → 4 NH3(g)+502(g) The reaction is endothermic. Suppose a mixture of NO, H,O, NH, and O, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium O to the right The temperature is lowered. O to the left The pressure of NH3 will ? O (none) O to the right to the left The temperature is raised. The pressure of H20 will ? O (none) O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Canter Acces Check Explanation 55 F Clear DELL Dele Insert PrtScrarrow_forwardPlease answer all parts.arrow_forward
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