Organic Chemistry
7th Edition
ISBN: 9780321803221
Author: Paula Y. Bruice
Publisher: Prentice Hall
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Textbook Question
Chapter 5.7, Problem 23P
a. for which reaction in each set will ∆S° be more significant?
b. for which reaction will ∆S° be positive?
- 1.
- 2.
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11. This reaction must have a ∆G>0 at SATP:
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1. 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?
Chapter 5 Solutions
Organic Chemistry
Ch. 5.1 - Determine the degree of unsaturation and then draw...Ch. 5.1 - Prob. 4PCh. 5.2 - Prob. 5PCh. 5.2 - Draw the structure for each of the following: a....Ch. 5.2 - What is each compounds systematic name?Ch. 5.4 - Assign relative priorities to each set of...Ch. 5.4 - Tamoxifen slows the growth of some breast tumors...Ch. 5.4 - Draw and label the E and Z isomers for each of the...Ch. 5.4 - Prob. 12PCh. 5.4 - Name each of the following:
Ch. 5.4 - Prob. 14PCh. 5.4 - Prob. 15PCh. 5.6 - Prob. 16PCh. 5.6 - Prob. 17PCh. 5.6 - Prob. 18PCh. 5.6 - Prob. 20PCh. 5.7 - a. Which of the monosubstituted cyclohexanes in...Ch. 5.7 - a. for which reaction in each set will S be more...Ch. 5.7 - a. For a reaction with H = 12 kcal/ mol and S =...Ch. 5.7 - Prob. 25PCh. 5.7 - Prob. 26PCh. 5.7 - Prob. 27PCh. 5.9 - The rate constant for a reaction can be increased...Ch. 5.9 - Prob. 30PCh. 5.9 - a. Which reaction has a greater equilibrium...Ch. 5.10 - Draw a reaction coordinate diagram for a two-step...Ch. 5.10 - a. Which step in the reaction coordinate diagram...Ch. 5.10 - Draw a reaction coordinate diagram for the...Ch. 5.11 - Prob. 35PCh. 5 - What is each compounds systematic name?Ch. 5 - Draw the structure of a hydrocarbon that has six...Ch. 5 - Draw the condensed structure for each of the...Ch. 5 - Prob. 39PCh. 5 - Prob. 40PCh. 5 - Name the following:Ch. 5 - Prob. 42PCh. 5 - 43. Draw the skeletal structure of...Ch. 5 - In a reaction in which reactant A is in...Ch. 5 - Which bond is stronger? Briefly explain why.Ch. 5 - Prob. 46PCh. 5 - Prob. 47PCh. 5 - Assign relative priorities to each set of...Ch. 5 - Prob. 49PCh. 5 - By following the curved red arrows, draw the...Ch. 5 - Prob. 51PCh. 5 - Draw structures for the following: a....Ch. 5 - Prob. 53PCh. 5 - a. Which of the following reactions has the larger...Ch. 5 - a. What is the equilibrium constant for a reaction...Ch. 5 - Prob. 56PCh. 5 - Prob. 57PCh. 5 - Given that the free energy of the twist-boat...Ch. 5 - Prob. 59PCh. 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
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- 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?arrow_forwardAn 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 reactionsarrow_forwardConsider 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_forward
- 24) 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_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 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_forwardConsider 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_forwardPRE-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_forward
- For 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: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_forwardCalculate the ∆S 0 for each given reaction. 1. 2H2 (g) + O2 (g) ---> 2H2O (g) 2. Ca3(PO4)2 (s) ---> 3Ca+2 (aq) + 2PO4 -3 (aq)arrow_forward
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