Pearson eText Organic Chemistry -- Instant Access (Pearson+)
8th Edition
ISBN: 9780135213711
Author: Paula Bruice
Publisher: PEARSON+
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 5.6, Problem 21P
a. for which reaction in each set will ∆S° be more significant?
b. for which reaction will ∆S° be positive?
- 1.
- 2.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
11. This reaction must have a ∆G>0 at SATP:
2O3(g)→3O2(g)
C(s)+O2(g)→CO2(g)
2K(s)+F2(g)→KF2(s)
2Fe2O3(s)→4Fe(s)+3O2(g)
For a reaction with ∆H° = -12 kcal>mol and ∆S° = 0.01 kcal mol-1 K-1, calculate the ∆G° and the equilibrium constant at: 1. 30 °C and 2. 150 °C. b. How does ∆G° change as T increases? c. How does Keq change as T increases?
An example of a reaction where ∆G = 0 is
a. any reaction that has reached completion
b. 2H2(g)+O2(g)→2H2O(g)
c. 2H2(g)+O2(g)→2H2O(l)
d. only reversible reactions
Chapter 5 Solutions
Pearson eText Organic Chemistry -- Instant Access (Pearson+)
Ch. 5.1 - What is the molecular formula for each of the...Ch. 5.1 - Prob. 4PCh. 5.1 - Determine the degree of unsaturation and then draw...Ch. 5.1 - Prob. 6PCh. 5.2 - What is each compounds systematic name?Ch. 5.2 - Prob. 8PCh. 5.2 - Draw the structure for each of the following: a....Ch. 5.3 - How many carbons are in the planar double-bond...Ch. 5.3 - Prob. 12PCh. 5.5 - Prob. 13P
Ch. 5.5 - Prob. 14PCh. 5.5 - Prob. 16PCh. 5.5 - Prob. 17PCh. 5.6 - a. Which of the monosubstituted cyclohexanes in...Ch. 5.6 - a. Calculate the percentage of isopropylcylohexane...Ch. 5.6 - a. for which reaction in each set will S be more...Ch. 5.6 - a. For a reaction with H = 12 kcal/ mol and S =...Ch. 5.8 - Prob. 23PCh. 5.9 - Prob. 24PCh. 5.9 - How many different alkenes can be hydrogenated to...Ch. 5.9 - The same alkane is obtained from the catalytic...Ch. 5.9 - Prob. 27PCh. 5.9 - Rank the following compounds from most stable to...Ch. 5.10 - Prob. 29PCh. 5.10 - Prob. 30PCh. 5.11 - The rate constant for a reaction can be increased...Ch. 5.11 - Prob. 33PCh. 5.11 - a. Which reaction has a greater equilibrium...Ch. 5.12 - Draw a reaction coordinate diagram for a two-step...Ch. 5.12 - a. Which step in the reaction coordinate diagram...Ch. 5.12 - Draw a reaction coordinate diagram for the...Ch. 5.13 - Prob. 38PCh. 5 - What is each compounds systematic name?Ch. 5 - Prob. 40PCh. 5 - Draw the structure of a hydrocarbon that has six...Ch. 5 - Draw the condensed structure for each of the...Ch. 5 - Prob. 43PCh. 5 - Prob. 44PCh. 5 - Prob. 45PCh. 5 - Name the following:Ch. 5 - Prob. 47PCh. 5 - Prob. 48PCh. 5 - Prob. 49PCh. 5 - In a reaction in which reactant A is in...Ch. 5 - Which bond is stronger? Briefly explain why.Ch. 5 - Prob. 52PCh. 5 - Prob. 53PCh. 5 - By following the curved red arrows, draw the...Ch. 5 - Prob. 55PCh. 5 - Prob. 56PCh. 5 - Draw structures for the following: a....Ch. 5 - Prob. 58PCh. 5 - a. Which of the following reactions has the larger...Ch. 5 - Prob. 60PCh. 5 - a. What is the equilibrium constant for a reaction...Ch. 5 - Prob. 62PCh. 5 - Prob. 63PCh. 5 - Given that the free energy of the twist-boat...Ch. 5 - Prob. 65PCh. 5 - Prob. 1PCh. 5 - Prob. 2PCh. 5 - Prob. 3PCh. 5 - Prob. 4PCh. 5 - Prob. 5PCh. 5 - Prob. 6PCh. 5 - Draw curved arrows to show the movement of the...Ch. 5 - Prob. 8PCh. 5 - Prob. 9PCh. 5 - Prob. 10P
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
- If the ∆S is calculated to be positive, there is greater disorder inthe, which would drive the reaction in the reaction? A. reactant (s), forward B. product (s), forward C. product (s), reverse D. reactant (s), reversearrow_forward1. Describe how you would calculate ∆G0′ for the reaction: glucose+ 6 O2 = 6 CO2 + 6 H2O. If you were told that this reaction is highlyexergonic, what would be the arithmetic sign (negative or positive)of the ∆G0′ you would expect for this reaction?arrow_forward24) Consider the following free energy curve for the reaction: A=B Pure A Pure B extent of reaction a) At equilibrium (2), is the system more enriched in A or in B? Provide a brief explanation of your choice. b) What would be the relative value of K? Greater than one, zero, or less than 1? Again, provide a brief explanation of your choice. free energyarrow_forward
- Consider the following reaction at equilibrium: N₂O₄(g) ⇌ 2NO₂(g) The ∆H° for this reaction is > 0. If the temperature is increased by 20.0 K while the volume is kept constant, in which direction will the equilibrium shift?arrow_forwardPredict the spontaneity of a reaction (and the temperaturedependence of the spontaneity) for each possible combination ofsigns for ∆H and ∆S (for the system).a. ∆H negative, ∆S positiveb. ∆H positive, ∆S negativec. ∆H negative, ∆S negatived. ∆H positive, ∆S positivearrow_forwardWhich of the following is a Nernst equation? a. ∆G = ∆Go + RT ln Q b. ∆Go = - RT ln K c. Eo = (RT/nF) ln K d. E = Eo - (RT/nF)ln Qarrow_forward
- Consider the data provided for the following rxn: H2O(l)⇌ H2O(g) a. Plot a graph and determine the ∆H and ∆S for the reaction. describe how they influence the spontaneity of the reaction as a function of temperature. T(°C): 0.0, 10.0, 20.0, 25.0, 30.0, 40.0, 60.0, 70.0, 90.0 P(torr): 4.579, 9.209, 17.53, 23.76, 31.82, 55.32, 149.4, 233.7, 525.8 b. explain how the boiling temperature of H2O(l) (at sea level) can be accurately determined from the data in a? c. for the reaction in a, ∆E is less than ∆H. Explain why.arrow_forwardFor a reaction carried out at 25 °C with an equilibrium constant of 1 x 10-3, to increase the equilibrium constant by a factor of 10: a. how much must ∆G° change? b. how much must ∆H° change if ∆S° = 0 kcal mol -1 K -1? c. how much must ∆S° change if ∆H° = 0 kcal mol -1?arrow_forwardConsider the following reaction at equilibrium: 2NO₂(g) ⇌ N₂O₄(g) The ∆H° for this reaction is < 0. If the volume of the container is decreased by ½ while the temperature is kept constant, how will K(eq) change?arrow_forward
- PRE-LABORATORY ASSIGNMENT You must finish the pre-laboratory assignments before beginning the laboratory experiment. 1. The following reaction is at equilibrium H₂(g) + CO₂(g) H₂O(g) + CO(g). a. I Determine the free energy change, AG°, at T = 298 K. b. If the partial pressures of H₂(g), CO₂(g), H₂O(g), and CO(g) are 20, 40, 0.04, and 0.02 atm, respectively, determine the free energy change as a function of temperature, AG°(T).arrow_forwardConsider the following reaction at equilibrium:2CO2 (g) --><-- 2CO (g) + O2 (g) ∆H° = -514 kJLe Châtelier's principle predicts that removing O2(g) to the reaction container will ________. Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g) + O2 (g) ∆H° = -514 kJ A. increase the partial pressure of CO2 B. decrease the partial pressure of CO C. increase the partial pressure of CO D. decrease the value of the equilibrium constant E. increase the value of the equilibrium constantarrow_forward44. If the reaction A + B = C has an equilibrium constant greater than 1, which of the following statements is correct concerning the forward reaction? A) The forward reaction is not thermodynamically favored and would be considered non-spontaneous. %3D B) The forward reaction rate is fast. C) The forward reaction is slow. D) The forward reaction is thermodynamically favored and would be considered spontaneous.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
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