CHEMISTRY LOOSELEAF TEXT W/CONNECT >IP
4th Edition
ISBN: 9781259936586
Author: Burdge
Publisher: MCG
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 18.5, Problem 1PPA
Practice Problem ATTEMPT
A reaction will be spontaneous only at low temperatures if both
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Compute ΔGo at 200.0 oC for each of the following reactions, which are important in the chemistry of coal. Assume that coal has the same thermodynamic properties as graphite.
Substance
ΔHo(kJ/mol)
So(J/(mol*K))
C(graphite)
0
5.7
H2O(g)
-241.83
188.835
CO(g)
-110.5
197.7
H2(g)
0
130.680
O2(g)
0
205.152
CO2(g)
-393.5
213.8
C(s, coal) + H2O(g) CO(g) + H2(g)
C(s, coal) + O2(g) CO2(g)
C(s, coal) + 1/2O2(g) CO(g)
CO(g) + H2O(g) CO2(g) + H2(g)
Consider the combustion of ethane:
2C2H6 + 7O2 --> 4CO2 + 6H2O
Substance
ΔHf
C2H6
-84.7
O2
0
CO2
-393.5
H2O
-242.0
What is ΔHcombustion (ΔHreaction) ?
Question 2 options:
550.8 kJ
-2856.6 kJ
2856.6 kJ
-550.8 kJ
5H. Based on the following practice problem, if either of the reactions is nonspontaneous but can become spontaneous, at what temperature might it become spontaneous? Round your answer to 2 significant digits.
Chapter 18 Solutions
CHEMISTRY LOOSELEAF TEXT W/CONNECT >IP
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...
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
- What is ΔH, ΔS and ΔG° at 1000 °C for the following reaction? CaCO3 (s) = CaO (s) + CO2 (g) ΔHf° (KJ) S° (J/K CaCO3 -1206.9 92.9 CaO -635.1 38.2 CO2 -393.5 213.7 ΔHAnswerKJ ΔSAnswerJ/K ΔGoAnswerKJ (b) Is the reaction spontaneous at 1000 °C and 1 atm? Answer (c) What is the value of Kp at 1000 °C for this reaction given that (R = 8.314 J/K mol) KpAnswer (d) What is the partial pressure of CO2 (g)?Answeratmarrow_forwardWhat is the work when a gas expands from 0.666 L to 2.334 L against an external pressure of 2.07 atm? Note: answer is in Joules.arrow_forwardSelect the circumstances under which a reaction would most likely be spontaneous. a. delta H is positive, delta S is positive, and the temperature is low. b. delta H is positive, delta S is negative, and the temperature is low. c. delta H is positive, delta S is negative, and the temperature is high. d. delta H is negative, delta S is negative, and the temperature is high. e. delta H is negative, delta S is positive, and the temperature is high.arrow_forward
- Which of the following processes are endothermic? Check all that apply. H2O(l) ⟶⟶ H2O(s) H2O(g) ⟶⟶ H2O(l) 2 C8H18(l) + 25 O2(g) ⟶⟶ 16 CO2(g) + 18 H2O(l) CO2(s) ⟶⟶ CO2(g) 2 H2(g) + O2(g) ⟶⟶ 2 H2O(g) Δ?=−241.83??ΔH=−241.83kJ 2 Al(s) + 1.5 O2 ⟶⟶ Al2O3 Δ?=−1675.7??ΔH=−1675.7kJ Br2(g) ⟶⟶ 2Br(g) 1/2 N2(g) + O2(g) ⟶⟶ NO2(g) Δ?=33.1??ΔH=33.1kJarrow_forward2 NO (g) + O₂ (g) → 2 NO₂ (g) At what temperature (in ºC) will the reaction change the direction in which it is spontaneous under standard pressure conditions? Please type answer note write by hendarrow_forwardCan the Kp and Kc for a reaction ever have the same value? Why or why not? Answer:arrow_forward
- The combination of ΔH and ΔS for a process that will always be nonspontaneous is _____. ΔH is positive and ΔS is positive ΔH is negative and ΔS is positive ΔH is negative and ΔS is negative ΔH is positive and ΔS is negativearrow_forwardFor which of the following is the change in entropy positive? Check all that apply. Explain. A. C 6 H 12 (l) C 6 H 12 (g)B. Dilution of 1.0 mL of 1.0 M NaOH with 90 mL of waterC. . 2 O 2 (g) + 2 SO (g) 2 SO 3 (g)D. grinding a large crystal of NaCl to powderE. Cooling water from room temperature to 15°C.arrow_forwardThe Gibbs free energy change (∆Go) of reaction A is 300 kJ/mol and that of reaction B is -400 kJ/mol. Which reaction is faster (A, B or impossible to determine with the given information)? Please explain answerarrow_forward
- Which statement is true for the freezing of liquid water below 0 °C? Group of answer choices ΔH is positive; ΔS is positive; ΔG is positive ΔH is positive; ΔS is negative; ΔG is positive ΔH is negative; ΔS is negative; ΔG is negative ΔH is positive; ΔS is negative; ΔG is negativearrow_forward(Question 2 reference: Use Hess’s law to calculate the amount of heat released when 10 g of ethanol C2H5OH is combusted with oxygen to form carbon dioxide and liquid water. (Molar mass of ethanol = 46 g/mol)) F 3. Calculate the change in entropy in J/K when 10g of ethanol are combusted as in question 2.arrow_forwardOut atmosphere is composed primarily of nitrogen and oxygen, which coexist at 25°C without reacting to any significant extent. However, the two gases can react to form nitrogen monoxide according to the following reaction: N2(g) + O2(g) ⇌ 2NO(g) Calculate delta G° at 1940K. (Express answer using four significant figures.) Does the reaction become spontaneous with increasing temperature?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 LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher: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 & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
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