EBK CHEMISTRY: ATOMS FIRST
3rd Edition
ISBN: 8220103675505
Author: Burdge
Publisher: YUZU
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Textbook Question
Chapter 14, Problem 14.62QP
Which of the following is not accompanied by an increase in the entropy of the system: (a) mixing of two gases at the same temperature and pressure, (b) mixing of ethanol and water, (c) discharging a battery, (d) expansion of a gas followed by compression to its original temperature, pressure, and volume?
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Chapter 14 Solutions
EBK CHEMISTRY: ATOMS FIRST
Ch. 14.3 - Determine the change in entropy for 1.0 mole of an...Ch. 14.3 - Determine the change in entropy (Ssys) for the...Ch. 14.3 - To what fraction of its original volume must a...Ch. 14.3 - From the standard entropy values in Appendix 2,...Ch. 14.3 - Prob. 2PPACh. 14.3 - In each of the following reactions, there is one...Ch. 14.3 - For each reaction shown in the diagrams, indicate...Ch. 14.3 - For each process, determine the sign of S for the...Ch. 14.3 - Prob. 3PPACh. 14.3 - Make a qualitative prediction of the sign of Hsoln...
Ch. 14.3 - Consider the gas-phase reaction of A2 (blue) and...Ch. 14.3 - Prob. 14.3.1SRCh. 14.3 - For which of the following chemical reactions is S...Ch. 14.3 - Prob. 14.3.3SRCh. 14.4 - Determine if each of the following is a...Ch. 14.4 - For each of the following, calculate Suniv and...Ch. 14.4 - (a) Calculate Suniv and determine if the reaction...Ch. 14.4 - The following table shows the signs of Ssys,...Ch. 14.4 - Using data from Appendix calculate S (in J/K mol)...Ch. 14.4 - Prob. 14.4.2SRCh. 14.4 - Prob. 14.4.3SRCh. 14.4 - Prob. 14.4.4SRCh. 14.4 - Prob. 14.4.5SRCh. 14.5 - According to Table 14 4, a reaction will be...Ch. 14.5 - A reaction will be spontaneous only at low...Ch. 14.5 - Given that the reaction 4Fe(s) + 3O2(g) + 6H2O(l) ...Ch. 14.5 - Prob. 5PPCCh. 14.5 - Prob. 14.6WECh. 14.5 - Prob. 6PPACh. 14.5 - For each reaction, determine the value of Gf that...Ch. 14.5 - Prob. 6PPCCh. 14.5 - Prob. 14.7WECh. 14.5 - Prob. 7PPACh. 14.5 - Prob. 7PPBCh. 14.5 - Prob. 7PPCCh. 14.5 - Prob. 14.5.1SRCh. 14.5 - Prob. 14.5.2SRCh. 14.5 - Prob. 14.5.3SRCh. 14 - Using Gf values from Appendix 2, calculate the...Ch. 14 - Prob. 14.2KSPCh. 14 - Using Grxnvalues from Appendix 2, calculate the...Ch. 14 - Prob. 14.4KSPCh. 14 - Explain what is meant by a spontaneous process....Ch. 14 - Which of the following processes are spontaneous...Ch. 14 - Prob. 14.3QPCh. 14 - Prob. 14.4QPCh. 14 - Prob. 14.5QPCh. 14 - Prob. 14.6QPCh. 14 - Prob. 14.7QPCh. 14 - Consider two gas samples at STP: one consisting of...Ch. 14 - Now consider the reaction F2(g)2F(g)at constant...Ch. 14 - Which of the following best describes why entropy...Ch. 14 - Which of the following best explains why entropy...Ch. 14 - How does the entropy of a system change for each...Ch. 14 - How does the entropy of a system change for each...Ch. 14 - Predict whether the entropy change is positive or...Ch. 14 - Prob. 14.11QPCh. 14 - Calculate Ssys for (a) the isothermal expansion of...Ch. 14 - Calculate Ssys for (a) the isothermal compression...Ch. 14 - Using the data in Appendix 2, calculate the...Ch. 14 - Using the data in Appendix 2, calculate the...Ch. 14 - For each pair of substances listed here, choose...Ch. 14 - Arrange the following substances (1 mole each) in...Ch. 14 - State the second law of thermodynamics in words,...Ch. 14 - State the third law of thermodynamics in words,...Ch. 14 - Calculate Ssurr for each of the reactions in...Ch. 14 - Calculate Ssurr for each of the reactions in...Ch. 14 - Using data from Appendix 2, calculate Srxn and...Ch. 14 - Using data from Appendix 2, calculate Srxn and...Ch. 14 - When a folded protein in solution is heated to a...Ch. 14 - Define free energy. What are its units?Ch. 14 - Why is it more convenient to predict the direction...Ch. 14 - What is the significance of the sign of Gsys?Ch. 14 - From the following combinations of H and S,...Ch. 14 - Prob. 14.29QPCh. 14 - Calculate G for the following reactions at 25C....Ch. 14 - Calculate G for the following reactions at 25C....Ch. 14 - From the values of H and S, predict which of the...Ch. 14 - Find the temperatures at which reactions with the...Ch. 14 - The molar heats of fusion and vaporization of...Ch. 14 - The molar heats of fusion and vaporization of...Ch. 14 - Use the values listed in Appendix 2 to calculate G...Ch. 14 - Certain bacteria in the soil obtain the necessary...Ch. 14 - What is a coupled reaction? What is its importance...Ch. 14 - What is the role of ATP in biological reactions?Ch. 14 - Prob. 14.40QPCh. 14 - Predict the signs of H, S, and G of the system for...Ch. 14 - A student placed 1 g of each of three compounds A,...Ch. 14 - The enthalpy change in the denaturation of a...Ch. 14 - Consider the following facts: Water freezes...Ch. 14 - Ammonium nitrate (NH4NO3) dissolves spontaneously...Ch. 14 - The standard enthalpy of formation and the...Ch. 14 - (a) Troutons rule states that the ratio of the...Ch. 14 - Referring to Problem 14.47, explain why the ratio...Ch. 14 - Prob. 14.49QPCh. 14 - Prob. 14.50QPCh. 14 - Prob. 14.51QPCh. 14 - Prob. 14.52QPCh. 14 - Prob. 14.53QPCh. 14 - The molar heat of vaporization of ethanol is 39 3...Ch. 14 - As an approximation, we can assume that proteins...Ch. 14 - When a native protein in solution is heated to a...Ch. 14 - A 74.6-g ice cube floats in the Arctic Sea. The...Ch. 14 - A reaction for which H and S are both negative is...Ch. 14 - The sublimation of carbon dioxide at 78C is given...Ch. 14 - Many hydrocarbons exist as structural isomers,...Ch. 14 - Consider the following reaction at 298 K. 2H2(s) +...Ch. 14 - Which of the following is not accompanied by an...Ch. 14 - Which of the following are not state functions: S,...Ch. 14 - Give a detailed example of each of the following,...Ch. 14 - Hydrogenation reactions (e.g., the process of...Ch. 14 - At 0 K. the entropy of carbon monoxide crystal is...Ch. 14 - Which of the following thermodynamic functions are...
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- Someone once suggested that it is impossible to unscramble a scrambled egg. Describe an unscrambled and a scrambled egg in terms of the concept of entropy.arrow_forwardExplain how the entropy of the universe increases when an aluminum metal can is made from aluminum ore. Thefirst step is to extract the ore, which is primarily a formof A12O3, from the ground. After it is purified by freeingit from oxides of silicon and iron, aluminum oxide ischanged to the metal by an input of electrical energy. 2Al2O3(s)electricalenergy4Al(s)+3O2(g)arrow_forwardConsider the reaction of 1 mol H2(g) at 25C and 1 atm with 1 mol Br2(l) at the same temperature and pressure to produce gaseous HBr 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
- Explain why absolute entropies can be measured.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_forwardFor the decomposition of formic acid, HCOOH(l)H2O(l)+CO(g) H = +29 kJ/mol at 25C. a Does the tendency of this reaction to proceed to a state of minimum energy favor the formation of water and carbon monoxide or formic acid? Explain. b Does the tendency of this reaction to proceed to a state of maximum entropy favor the formation of products or reactants? Explainarrow_forward
- For each process, tell whether the entropy change of the system is positive or negative, (a) A glassblower heats glass (the system) to its softening temperature, (b) A teaspoon of sugar dissolves in a cup of coffee. (The system consists of both sugar and coffee.) (c) Calcium carbonate precipitates out of water in a cave to form stalactites and stalagmites. (Consider only the calcium carbonate to be the system.)arrow_forwardWhat is entropy? Why is entropy important?arrow_forwardSuppose you have four identical molecules labeled 1, 2, 3, and 4. Draw 16 simple two-flask diagrams as in thefigure for Question 17, and draw all possible arrangements of the four molecules in the two flasks. How manyof these arrangements have two molecules in each flask?How many have no molecules in one flask? From theseresults, what is the most probable arrangement of molecules? Which arrangement has the highest entropy?arrow_forward
- At room temperature, the entropy of the halogens increases from I2 to Br2 to Cl2. Explain.arrow_forwardTetrachloromethane (carbon tetrachloride), CCl4, has a normal boiling point of 76.7C and an enthalpy of vaporization, Hvap, of 29.82 kJ/mol. Estimate the entropy of vaporization, Svap. Estimate the free energy of vaporization, Gvap, at 25C.arrow_forwardFor each process, tell whether the entropy change of the system is positive or negative. (a) A glassblower heats glass (the system) to its softening temperature. (b) A teaspoon of sugar dissolves in a cup of coffee. (The system consists of both sugar and coffee.) (c) Calcium carbonate precipitates out of water in a cave to form stalactites and stalagmites. (Consider only the calcium carbonate to be the system.)arrow_forward
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