Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 18, Problem 44GQ
Using
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Methane and chlorine react to form chloroform and hydrogen chloride, like
this:
CH,(g)+3C1,(g) → CHCI,(g)+3HC1(g)
The reaction is exothermic. Suppose a mixture of cCH, Cl, CHCI, and HCi 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.
olo
perturbation
change in composition
shift in equilibrium
O to the right
The temperature is
lowered.
O to the left
The pressure of CHCI3 will ?
O (none)
O to the right
O to the left
The temperature is raised. The pressure of Cl2 will
O (none)
Methane and chlorine react to form chloroform and hydrogen chloride, like this:
CH4(g) + 3Cl₂(g) → CHC13(g) + 3HCl(g)
The reaction is exothermic. Suppose a mixture of CH4, C1₂, CHC13 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
The temperature is
lowered.
change in composition
The pressure of CH4 will
The temperature is raised. The pressure of CHCl3 will
✓ ?
go up.
go down.
not change.
?
↑
shift in equilibrium
O
X
to the right
to the left
(none)
to the right
to the left
(none)
Ś
Methane 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
hp
Chapter 18 Solutions
Chemistry & Chemical Reactivity
Ch. 18.1 - 1. A process is spontaneous in the direction that...Ch. 18.1 - A process that is reactant-favored at equilibrium...Ch. 18.1 - Prob. 3RCCh. 18.2 - In a spontaneous process, S(universe) is (a) 0 (b)...Ch. 18.2 - 2. Which of the following is true for a...Ch. 18.2 - Prob. 3RCCh. 18.3 - Prob. 1RCCh. 18.3 - Prob. 2RCCh. 18.4 - Predict which substance in each pair has the...Ch. 18.4 - Prob. 2CYU
Ch. 18.4 - Without looking up their standard entropies in...Ch. 18.4 - Without doing any calculations, predict the sign...Ch. 18.4 - Calculate rS for the following reaction at 25 C....Ch. 18.5 - Based on rH and rS, predict the spontaneity of the...Ch. 18.5 - Prob. 1RCCh. 18.5 - Prob. 2RCCh. 18.5 - Prob. 3RCCh. 18.6 - Prob. 1RCCh. 18.6 - Prob. 2RCCh. 18.7 - Prob. 1CYUCh. 18.7 - Prob. 2CYUCh. 18.7 - Oxygen was first prepared by Joseph Priestley...Ch. 18.7 - Prob. 4CYUCh. 18.7 - Prob. 5CYUCh. 18.7 - Prob. 6CYUCh. 18.7 - Prob. 1RCCh. 18.7 - Prob. 2RCCh. 18.7 - Prob. 3RCCh. 18.7 - Consider the hydrolysis reactions of creatine...Ch. 18.7 - Prob. 2QCh. 18.A - The decomposition of diamond to graphite...Ch. 18.A - It has been demonstrated that buckminsterfullerene...Ch. 18 - Which substance has the higher entropy? (a) dry...Ch. 18 - Which substance has the higher entropy? (a) a...Ch. 18 - Use S values to calculate the standard entropy...Ch. 18 - Use S values to calculate the standard entropy...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Calculate the standard entropy change for the...Ch. 18 - Is the reaction Si(s) + 2 Cl2(g) SiCl4(g)...Ch. 18 - Is the reaction Si(s) + 2 H2(g) SiH4(g)...Ch. 18 - Calculate S(universe) for the decomposition of 1...Ch. 18 - Calculate S(universe) for the formation of 1 mol...Ch. 18 - Classify each of the reactions according to one of...Ch. 18 - Classify each of the reactions according to one of...Ch. 18 - Using values of fH and S, calculate rG for each of...Ch. 18 - Using values of fH and S, calculate rG for each of...Ch. 18 - Using values of fH and S, calculate the standard...Ch. 18 - Using values of fH and S, calculate the standard...Ch. 18 - Using values of fG, calculate rG for each of the...Ch. 18 - Using values of fG, calculate rG for each of the...Ch. 18 - For the reaction BaCO3(s) BaO(s) + CO2(g), rG =...Ch. 18 - For the reaction TiCl2(s) + Cl2(g) TiCl4(), rG =...Ch. 18 - Determine whether the reactions listed below are...Ch. 18 - Determine whether the reactions listed below are...Ch. 18 - Heating some metal carbonates, among them...Ch. 18 - Calculate rH and rS for the reaction of tin(IV)...Ch. 18 - The standard free energy change, rG, for the...Ch. 18 - Prob. 28PSCh. 18 - Calculate rG at 25 C for the formation of 1.00 mol...Ch. 18 - Prob. 30PSCh. 18 - Prob. 31PSCh. 18 - Prob. 32PSCh. 18 - Compare the compounds in each set below and decide...Ch. 18 - Using standard entropy values, calculate rS for...Ch. 18 - About 5 billion kilograms of benzene, C6H6, are...Ch. 18 - Hydrogenation, the addition of hydrogen to an...Ch. 18 - Is the combustion of ethane, C2H6, product-favored...Ch. 18 - Prob. 38GQCh. 18 - When vapors from hydrochloric acid and aqueous...Ch. 18 - Calculate S(system), S(surroundings), and...Ch. 18 - Methanol is now widely used as a fuel in race...Ch. 18 - The enthalpy of vaporization of liquid diethyl...Ch. 18 - Calculate the entropy change, rS, for the...Ch. 18 - Using thermodynamic data, estimate the normal...Ch. 18 - Prob. 45GQCh. 18 - When calcium carbonate is heated strongly, CO2 gas...Ch. 18 - Sodium reacts violently with water according to...Ch. 18 - Yeast can produce ethanol by the fermentation of...Ch. 18 - Elemental boron, in the form of thin fibers, can...Ch. 18 - Prob. 50GQCh. 18 - Prob. 51GQCh. 18 - Estimate the boiling point of water in Denver,...Ch. 18 - The equilibrium constant for the butane ...Ch. 18 - A crucial reaction for the production of synthetic...Ch. 18 - Calculate rG for the decomposition of sulfur...Ch. 18 - Prob. 56GQCh. 18 - A cave in Mexico was recently discovered to have...Ch. 18 - Wet limestone is used to scrub SO2 gas from the...Ch. 18 - Sulfur undergoes a phase transition between 80 and...Ch. 18 - Calculate the entropy change for dissolving HCl...Ch. 18 - Some metal oxides can be decomposed to the metal...Ch. 18 - Prob. 62ILCh. 18 - Prob. 63ILCh. 18 - Prob. 64ILCh. 18 - Titanium(IV) oxide is converted to titanium...Ch. 18 - Cisplatin [cis-diamminedichloroplatinum(II)] is a...Ch. 18 - Prob. 67SCQCh. 18 - Explain why each of the following statements is...Ch. 18 - Decide whether each of the following statements is...Ch. 18 - Under what conditions is the entropy of a pure...Ch. 18 - Prob. 71SCQCh. 18 - Consider the formation of NO(g) from its elements....Ch. 18 - Prob. 73SCQCh. 18 - The normal melting point of benzene, C6H6, is 5.5...Ch. 18 - Prob. 75SCQCh. 18 - For each of the following processes, predict the...Ch. 18 - Heater Meals are food packages that contain their...Ch. 18 - Prob. 78SCQCh. 18 - Prob. 79SCQCh. 18 - Prob. 80SCQCh. 18 - Iodine, I2, dissolves readily in carbon...Ch. 18 - Prob. 82SCQCh. 18 - Prob. 83SCQCh. 18 - Prob. 84SCQCh. 18 - Prob. 85SCQCh. 18 - Prob. 86SCQCh. 18 - The Haber-Bosch process for the production of...Ch. 18 - Prob. 88SCQ
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 entropy? Why is entropy important?arrow_forwardWhen (if ever) are high temperatures unfavorable to a reaction thermodynamically?arrow_forwardIndicate whether each statement below is true or false. If a statement is false, rewrite it to produce a closely related statement that is true. For a given reaction, the magnitude of the equilibrium constant is independent of temperature. If there is an increase in entropy and a decrease in enthalpy when reactants in their standard states are converted to products in their standard states, the equilibrium constant for the reaction must be negative. The equilibrium constant for the reverse of a reaction is the reciprocal of the equilibrium constant for the reaction itself. For the reaction H2O2(ℓ) ⇌ H2O(ℓ) + O2(g) the equilibrium constant is one half the magnitude of the equilibrium constant for the reaction 2H2O2(ℓ) ⇌ 2H2O(ℓ) + O2(g)arrow_forward
- Industrially, methanol is synthesized using the reaction CO(g) + 2 H2(g) CH3OH(g) Calculate the equilibrium constant at 298 K. ΔGfo CO(g) = −137.2 kJ/mol; ΔGfo H2 (g)= 0 ; ΔGfo CH3OH(g) = -162 kJ/molarrow_forwardFor a certain chemical reaction, the standard Gibbs free energy of reaction at 5.00 °C is 92.4 kJ. Calculate the equilibrium constant K for this reaction. Round your answer to 2 significant digits.arrow_forwardFor a certain chemical reaction, the standard Gibbs free energy of reaction is -104. kJ. Calculate the temperature at which the equilibrium constant Round your answer to the nearest degree. 團 ?.arrow_forward
- Using Le Chatelier's Principle to predict the result of changing... Ammonia and oxygen react to form nitrogen and water, like this: 4NH3 (g)+30₂ (g) 2N₂(g)+6H₂O(g) Suppose a mixture of NH3, O2, N₂ and H₂O 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 Some NH3 is added. Some H₂O is removed. change in composition The pressure of O₂ will The pressure of N₂ will The pressure of NH3 will ? ? ? shift in equilibrium to the right to the left O (none) to the right to the leftarrow_forward14. In the reaction 2NO, (g) + energy 2NO (g) + 0, (g), what shift would occur if more oxygen gas were added to the closed system? Why? 15. How many total moles of reactants and how many total moles of products are in the reaction 2NO, (g) + energy 2NO (g) + O2 (g)? 16. If the pressure of the reaction system of 2No, (g) + energy 2NO (g) + 0, (g) is increased, the pressure is decreased, the favored. (forward or reverse) reaction will be favored. If the (forward or reverse) reaction will bearrow_forward6. The normal boiling point of rhothanol is 70 °C. Given that the vapor pressure of rhothanol is 68.6 torr at 16.8 °C, calculate the molar enthalpy of vaporization of rhothanol.arrow_forward
- Consider the following reaction at 298 K. 2 SO₂(g) + O₂(g) → 2 SO 3(g) An equilibrium mixture contains O₂(g) and SO3(g) at partial pressures of 0.58 atm and 2.6 atm, respectively. Using data from the Thermodynamic Data table, determine the equilibrium partial pressure of SO₂ in the mixture. atm Will this reaction be most favored at a high or a low temperature, assuming standard conditions? Ohigh temperature O low temperaturearrow_forwardConsider the following reaction at 298 K. 2 SO₂(g) + O₂(g) → 2 SO 3(g) An equilibrium mixture contains O₂(g) and SO3(g) at partial pressures of 0.57 atm and 2.5 atm, respectively. Using data from the Thermodynamic Data table, determine the equilibrium partial pressure of SO₂ in the mixture. atm Will this reaction be most favored at a high or a low temperature, assuming standard conditions? O high temperature O low temperaturearrow_forwardUp, down or centerarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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