CHEMISTRY >CUSTOM<
14th Edition
ISBN: 9781259137815
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Chapter 18, Problem 32QP
The molar heats of fusion and vaporization of ethanol are
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Chapter 18 Solutions
CHEMISTRY >CUSTOM<
Ch. 18.1 - Practice Problem ATTEMPT
Determine the change in...Ch. 18.1 - Practice Problem BUILD To what fraction of its...Ch. 18.1 - Practice Problem CONCEPTUALIZE
Which equation is...Ch. 18.2 - Practice ProblemATTEMPT Calculate the standard...Ch. 18.2 - Practice Problem BUILD
In each of the following...Ch. 18.2 - Practice Problem CONCEPTUALIZE
For each reaction...Ch. 18.3 - Practice ProblemATTEMPT For each of the following...Ch. 18.3 - Practice Problem BUILD
Make a qualitative...Ch. 18.3 - Practice Problem CONCEPTUALIZE
Consider the...Ch. 18.3 - 18.3.1 For which of the following physical...
Ch. 18.3 - 18.3.2 For which of the following chemical...Ch. 18.3 - 18.3.3 Identify the correct balanced equation and...Ch. 18.4 - Practice Problem ATTEMPT For each of the...Ch. 18.4 - Practice Problem BUILD (a) Calculate Δ S univ and...Ch. 18.4 - Practice Problem CONCEPTUALIZE The following table...Ch. 18.4 - Using data from Appendix 2, calculate Δ S ° (in...Ch. 18.4 - 18.4.2 Using data from Appendix 2, calculate (in...Ch. 18.4 - The diagrams show a spontaneous chemical reaction....Ch. 18.4 - 18.4.4 The diagrams show a spontaneous chemical...Ch. 18.5 - Practice Problem ATTEMPT
A reaction will be...Ch. 18.5 - Practice Problem BUILD
Given that the reaction is...Ch. 18.5 - Practice ProblemCONCEPTUALIZE Which of the...Ch. 18.5 - A reaction for which Δ H and Δ S are both negative...Ch. 18.5 - At what temperature ( in ºC ) does a reaction go...Ch. 18.5 - 18.5.3 Using data from Appendix 2, calculate G°...Ch. 18.5 - 18.5.4 Calculate for the sublimation of iodine in...Ch. 18.6 - Practice Problem ATTEMPT
Calculate the standard...Ch. 18.6 - Practice problemBUILD For each reaction, determine...Ch. 18.6 - Prob. 1PPCCh. 18.6 - 18.6.1 For the reaction:
Ch. 18.6 - Consider the reaction: X ( g ) + Y(g) ⇄ Z( g ) for...Ch. 18.6 - The Δ G° for the reaction: N 2 ( g ) + 3H 2 (g) ⇄...Ch. 18.6 - 18.6.4 The for iron(III) hydroxide . For the...Ch. 18.7 - Practice Problem ATTEMPT
The molar heats of fusion...Ch. 18.7 - Practice Problem CONCEPTUALIZE
Explain why. in...Ch. 18.8 - Practice ProblemATTEMPT Δ G ° for the reaction: H...Ch. 18.8 - Practice ProblemBUILD What is the minimum partial...Ch. 18.8 - Practice Problem CONCEPTUALIZE Consider the...Ch. 18.9 - Practice Problem ATTEMPT Using data from Appendix...Ch. 18.9 - Practice ProblemBUILD K f for the complex ion Ag (...Ch. 18.9 - Practice Problem CONCEPTUALIZE Which of the...Ch. 18.10 - Practice ProblemATTEMPT Calculate G for the...Ch. 18.10 - Practice ProblemBUILD Ksp for Co(OH)2 at...Ch. 18.10 - Prob. 1PPCCh. 18 - 18.1
Which of the following must be negative for a...Ch. 18 - Δ G for a reaction is always negative when (a) Δ G...Ch. 18 - 18.3
The diagram shown here depicts a system at...Ch. 18 - The reaction shown here has Δ G º = -1 .83 kJ/mol...Ch. 18 - 18.1 Explain what is meant by a spontaneous...Ch. 18 - Prob. 2QPCh. 18 - Prob. 3QPCh. 18 - Describe what is meant by the term entropy. What...Ch. 18 - Prob. 5QPCh. 18 - Prob. 6QPCh. 18 - Prob. 7QPCh. 18 - Prob. 8QPCh. 18 - How does the entropy of a system change for each...Ch. 18 - Prob. 10QPCh. 18 - Prob. 11QPCh. 18 - Prob. 12QPCh. 18 - Prob. 13QPCh. 18 - Using the data in Appendix 2, calculate the...Ch. 18 - 18.15 Using the data in Appendix 2, calculate the...Ch. 18 - Prob. 16QPCh. 18 - Prob. 17QPCh. 18 - Prob. 18QPCh. 18 - 18.19 State the third law of thermodynamics in...Ch. 18 - Calculate Δ S surr for each of the reactions in...Ch. 18 - Calculate Δ S surr for each of the reactions in...Ch. 18 - Using data from Appendix 2, calculate Δ S rxn º...Ch. 18 - 18.23 Using data from Appendix 2, calculate for...Ch. 18 - Prob. 24QPCh. 18 - Why is it more convenient to predict the direction...Ch. 18 - What is the significance of the sign of Δ G sys ?Ch. 18 - From the following combinations of Δ H and Δ S ,...Ch. 18 - Prob. 28QPCh. 18 - Prob. 29QPCh. 18 - From the values of Δ H and Δ S , predict which of...Ch. 18 - Find the temperatures at which reactions with the...Ch. 18 - The molar heats of fusion and vaporization of...Ch. 18 - 18.33 The molar heats of fusion and vaporization...Ch. 18 - Prob. 34QPCh. 18 - Prob. 35QPCh. 18 - Prob. 36QPCh. 18 - Prob. 37QPCh. 18 - Prob. 38QPCh. 18 - Explain why Equation 18.14 is of great importance...Ch. 18 - Prob. 40QPCh. 18 - Prob. 41QPCh. 18 - Prob. 42QPCh. 18 - 18.43 Consider the following reaction at...Ch. 18 - Prob. 44QPCh. 18 - 18.45
(a)
Calculate and for the following...Ch. 18 - Prob. 46QPCh. 18 - Consider the decomposition of calcium carbonate:...Ch. 18 - Prob. 48QPCh. 18 - 18.49 At for the process:
is 8.6 kJ/mol....Ch. 18 - Prob. 50QPCh. 18 - What is a coupled reaction? What is its importance...Ch. 18 - What is the role of ATP in biological reactions?Ch. 18 - Prob. 53QPCh. 18 - 18.54 In the metabolism of glucose, the first step...Ch. 18 - Predict the signs of Δ H , Δ S , and Δ G of the...Ch. 18 - Prob. 56APCh. 18 - Prob. 57APCh. 18 - Prob. 58APCh. 18 - Prob. 59APCh. 18 - Prob. 60APCh. 18 - Ammonium nitrate ( NH 4 NO 3 ) dissolves...Ch. 18 - 18.62 Calculate the equilibrium pressure of due...Ch. 18 - Prob. 63APCh. 18 - Referring to Problem 18.63, explain why the ratio...Ch. 18 - 18.65 Which of the following are not state...Ch. 18 - 18.66 For reactions carried out under...Ch. 18 - Prob. 67APCh. 18 - Prob. 68APCh. 18 - A student looked up the Δ G f o , Δ H f o , and Δ...Ch. 18 - Consider the following Brønsted acid-base reaction...Ch. 18 - 18.71 At o K, the entropy of carbon monoxide...Ch. 18 - Prob. 72APCh. 18 - Consider the thermal decomposition of CaCO 3 :...Ch. 18 - Prob. 74QPCh. 18 - Prob. 75QPCh. 18 - Prob. 76QPCh. 18 - Prob. 77APCh. 18 - Prob. 78APCh. 18 - Prob. 79APCh. 18 - Prob. 80APCh. 18 - Prob. 81APCh. 18 - Prob. 82APCh. 18 - 18.83 Comment on the statement: “Just talking...Ch. 18 - Prob. 84APCh. 18 - Consider the reaction: N 2 ( g ) + O 2 ( g ) ⇄ 2...Ch. 18 - Prob. 86APCh. 18 - Consider the decomposition of magnesium carbonate:...Ch. 18 - Prob. 88APCh. 18 - Prob. 89APCh. 18 - 18.90 The rate constant for the elementary...Ch. 18 - A 74.6-g ice cube floats in the Arctic Sea. The...Ch. 18 - 18.92 Which of the following is not accompanied by...Ch. 18 - Prob. 93APCh. 18 - Give a detailed example of each of the following,...Ch. 18 - Prob. 95QPCh. 18 - 18.96 The standard enthalpy of formation and the...Ch. 18 - Prob. 97QPCh. 18 - Prob. 98QPCh. 18 - The following reaction was described as the cause...Ch. 18 - Comment on the feasibility of extracting copper...Ch. 18 - 18.101 One of the steps in the extraction of iron...Ch. 18 - Prob. 102APCh. 18 - Prob. 103APCh. 18 - Prob. 104APCh. 18 - 18.105 The enthalpy change in the denaturation of...Ch. 18 - Prob. 106APCh. 18 - Prob. 107APCh. 18 - Prob. 108APCh. 18 - Prob. 109APCh. 18 - Prob. 110APCh. 18 - 18.111 Carbon monoxide and nitric oxide are...Ch. 18 - Prob. 112APCh. 18 - Prob. 113APCh. 18 - 18.114 Many hydrocarbons exist as structural...Ch. 18 - Physical and Biological Sciences
In chemistry, the...Ch. 18 - Physical and Biological Sciences
In chemistry, the...Ch. 18 - Prob. 3SEPPCh. 18 - Physical and Biological Sciences
In chemistry, the...
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- What is entropy? Why is entropy important?arrow_forwardDefine the term entropy, and give an example of a sample of matter that has zero entropy. What are the units of entropy? How do they differ from the units of enthalpy?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
- When most biological enzymes are heated, they lose their catalytic activity. This process is called denaturing. The change original enzyme new form that occurs on heating is endothermic and spontaneous. Is the structure of the original enzyme or its new form more ordered (has the smaller positional probability)? Explain.arrow_forwardWhich contains greater entropy, a quantity of frozen benzene or the same quantity of liquid benzene at the same temperature? Explain in terms of the dispersal of energy in the substance.arrow_forwardThe standard molar entropy of iodine vapor, I2(g), is 260.7 J Kl mol-1 and the standard molar enthalpy of formation is 62.4 kJ/mol. a) Calculate the entropy change for vaporization of 1 mol of solid iodine (use data from Table 16.1 or Appendix J). b) Calculate the enthalpy change for sublimation of iodine. c) Assuming that rSdoes not change with temperature, estimate the temperature at which iodine would sublime (change directly from solid to gas).arrow_forward
- Solid NH4NO3 is placed in a beaker containing water at 25 C. When the solid has completely dissolved, the temperature of the solution is 23.5 C. (a) Was the process exothermic or endothermic? (b) Was the process spontaneous? (c) Did the entropy of the system increase? (d) Did the entropy of the universe increase?arrow_forwardWhat happens to the entropy of the universe during a spontaneous process?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
- 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_forwardEnthalpy changes often help predict whether or not a process will be spontaneous. What type of reaction is more likely to be spontaneous: an exothermic or an endothermic one? Provide two examples that support your assertion and one counterexample.arrow_forwardThermodynamics 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_forward
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