Organic Chemistry Study Guide and Solutions
6th Edition
ISBN: 9781936221868
Author: Marc Loudon, Jim Parise
Publisher: W. H. Freeman
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Chapter 3, Problem 3.26P
Interpretation Introduction
(a)
Interpretation:
The correct number corresponding to the blank is to be stated.
Concept introduction:
The product of natural log of equilibrium constant, gas constant and specific temperature gives the value of free energy for the reaction. Free energy of a reaction is expressed in
Interpretation Introduction
(b)
Interpretation:
The correct number corresponding to the blank is to be stated.
Concept introduction:
The product of natural log of equilibrium constant, gas constant and specific temperature gives the value of free energy for the reaction. Free energy of a reaction is expressed in
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a) For the reaction given in Part A, how much heat is absorbed when 2.70 mol of AA reacts? (the image attached)
b) For the reaction given in Part A, ΔS∘rxn is 39.0 J/K . What is the standard Gibbs free energy of the reaction, ΔG∘rxn?
A student determines the value of the equilibrium constant to be 2.57×10-10 for the following reaction.
Fe2O3(s) + 3H2(g)2Fe(s) + 3H½0(g)
Based on this value of Keg:
AG° for this reaction is expected to be (greater, less)
than zero.
Calculate the free energy change for the reaction of 1.71 moles of Fe,O3(s) at standard conditions at 298K.
AG°
kJ
rxn
(a) The equilibrium constant of the isomerization of cis-2-butene to trans-2-butene is 2.07 at
127.0 °C. Determine the standard molar Gibbs free energy, AGR º for the reaction.
(b) For C6o, the standard molar Gibbs free energy (AG, º) of formation from the elemental carbon
is 23.98 kJ/mol at 25.0 °C. Determine the equilibrium constant, Keq for the formation of C60.
Chapter 3 Solutions
Organic Chemistry Study Guide and Solutions
Ch. 3 - Prob. 3.1PCh. 3 - Prob. 3.2PCh. 3 - Prob. 3.3PCh. 3 - Prob. 3.4PCh. 3 - Prob. 3.5PCh. 3 - Prob. 3.6PCh. 3 - Prob. 3.7PCh. 3 - Prob. 3.8PCh. 3 - Prob. 3.9PCh. 3 - Prob. 3.10P
Ch. 3 - Prob. 3.11PCh. 3 - Prob. 3.12PCh. 3 - Prob. 3.13PCh. 3 - Prob. 3.14PCh. 3 - Prob. 3.15PCh. 3 - Prob. 3.16PCh. 3 - Prob. 3.17PCh. 3 - Prob. 3.18PCh. 3 - Prob. 3.19PCh. 3 - Prob. 3.20PCh. 3 - Prob. 3.21PCh. 3 - Prob. 3.22PCh. 3 - Prob. 3.24PCh. 3 - Prob. 3.25PCh. 3 - Prob. 3.26PCh. 3 - Prob. 3.27PCh. 3 - Prob. 3.28PCh. 3 - Prob. 3.29PCh. 3 - Prob. 3.30PCh. 3 - Prob. 3.31PCh. 3 - Prob. 3.32APCh. 3 - Prob. 3.33APCh. 3 - Prob. 3.34APCh. 3 - Prob. 3.35APCh. 3 - Prob. 3.36APCh. 3 - Prob. 3.37APCh. 3 - Prob. 3.38APCh. 3 - Prob. 3.39APCh. 3 - Prob. 3.40APCh. 3 - Prob. 3.41APCh. 3 - Prob. 3.42APCh. 3 - Prob. 3.43APCh. 3 - Prob. 3.44APCh. 3 - Prob. 3.45APCh. 3 - Prob. 3.46APCh. 3 - Prob. 3.47APCh. 3 - Prob. 3.48APCh. 3 - Prob. 3.49APCh. 3 - Prob. 3.50APCh. 3 - Prob. 3.51APCh. 3 - Prob. 3.52APCh. 3 - Prob. 3.53APCh. 3 - Prob. 3.54APCh. 3 - Prob. 3.55APCh. 3 - Prob. 3.56APCh. 3 - Prob. 3.57APCh. 3 - Prob. 3.58APCh. 3 - Prob. 3.59APCh. 3 - Prob. 3.60AP
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- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forwarda Calculate K1, at 25C for phosphoric acid: H3PO4(aq)H+(aq)+H2PO4(aq) b Which thermodynamic factor is the most significant in accounting for the fact that phosphoric acid is a weak acid? Why ?arrow_forwardAnother step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.arrow_forward
- What information can be determined from G for a reaction? Does one get the same information from G, the standard free energy change? G allows determination of the equilibrium constant K for a reaction. How? How can one estimate the value of K at temperatures other than 25C for a reaction? How can one estimate the temperature where K = 1 for a reaction? Do all reactions have a specific temperature where K = 1?arrow_forwardAt room temperature, the equilibrium constant (Kw) for the self-ionization of water is 1.00 × 10−14. Using this information, calculate the standard free energy change for the aqueous reaction of hydrogen ion with hydroxide ionto produce water. (Hint: The reaction is the reverse of the self-ionization reaction.)arrow_forwardA student determines the value of the equilibrium constant to be 2.22x10 2 for the following reaction. CH (g) + H,O(g) →3H2(g) + CO(g) Based on this value of Keg AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.05 moles of CH,(g) at standard conditions at 298K. AG°. Ixn kJarrow_forward
- A student determines the value of the equilibrium constant to be 8.55×10-31 for the following reaction. N₂(g) + O₂(g)- >2NO(g) Based on this value of Keq: AG° for this reaction is expected to be (greater,less) Calculate the free energy change for the reaction of 1.89 moles of N₂(g) at standard conditions at 298K. AGᵒrxn kJ = than zero.arrow_forward1/2 Cl2 (g) -><- Cl (g) The reaction Gibbs free energies at various temperatures are given. A) Calculate the standard enthalpy change H ° of the reaction. B) Find the equilibrium constant of the reaction at a temperature of 1568 Kelvin? C) If 1.0 moles of Cl2 gas is heated to a temperature of 1568 Kelvin, how many moles of Cl are formed when the system equilibrates?arrow_forward
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