Guided course 05:02Breaking down the different terms of the Gibbs Free Energy equation.Johnny Betancourt1789views27rank7comments
Multiple Choice If ΔG° for a particular reaction is < 0 kcal/mol, which side of the reaction is favored?314views
Multiple Choice If a particular acid/base reaction has a Keq = 1027, how will ΔG° vary with temperature?325views
Textbook Question(•••) Looking ahead In Chapter 5, we explain that the equilibrium constant (Kₑ_q) for a reaction can be calculated based on the difference in energy between reactants and products, according to the following equation: Kₑ_q = e ^ -∆E/RT Using this equation, calculate the equilibrium constant for the 'reaction' shown. [For the rest of the book, if not otherwise specified, assume room temperature (298K).]356views
Textbook QuestionThe following reaction has a value of ΔG= -2.1 kJ/mol (-0.50 kcal/mol). CH3Br + H2S ⇌ CH3SH + HBr a. Calculate Keq at room temperature (25 °C) for this reaction as written.667views
Textbook QuestionThe following reaction has a value of ΔG= -2.1 kJ/mol (-0.50 kcal/mol). CH3Br + H2S ⇌ CH3SH + HBr b. Starting with a 1 M solution of CH3Br and H2S, calculate the final concentrations of all four species at equilibrium.489views
Textbook Questiona. Which reaction has a greater equilibrium constant: one with a rate constant of 1 * 10-3 sec-1 for the forward reaction and a rate constant of 1 * 10-5 sec-1 for the reverse reaction, or one with a rate constant of 1 * 10-2 sec-1 for the forward reaction and a rate constant of 1 * 10-3 sec-1 for the reverse reaction? b. If both reactions start with a reactant concentration of 1.0 M, which reaction will form the most product when the reactions have reached equilibrium?672views
Textbook QuestionThe rate of the reaction of methyl chloride with hydroxide ion is linearly dependent on both the concentration of methyl chloride and the concentration hydroxide ion. At 30 °C, the constant (k) for the reaction is 1.0 * 10-5 M-1 s-1 b. If the concentration of methyl chloride is decreased to 0.010 M, what will be the effect on 1. the rate of the reaction? 2. the rate constant for the reaction?461views
Textbook Questiona. For a reaction with ∆H° = -12 kcal>mol and ∆S° = 0.01kcal 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?388views
Textbook Question(••••) We discuss the following reaction in Chapters 12 and 13. (b) Mechanistically, the reaction occurs as shown below. Why is this reaction favored? Based on the stability of the anions, estimate K_eq.409views
Textbook QuestionFor the following equilibrium processes and the corresponding ∆G° , indicate whether you expect the equilibrium constant to be greater than, equal to, or less than 1. Justify your expectation in words. (a)351views
Textbook QuestionFor the following values of ∆H° , ∆S°, and T, tell whether the process would be favored. (c) ∆H° = -21.3 kcal/mol ; AS° = -51 cal/mol•K ; T = 373 K357views
Textbook QuestionA certain process has ∆H° = 11.7 kcal/mol and AS° = +33cal/mol•K . That is, this reaction has an unfavorable enthalpy but a favorable entropy term. At what temperature will the process be neither favored nor disfavored?302views
Textbook QuestionCalculate ∆G°, ∆H°, and ∆S° for the following acid–base reactions. Rationalize the value of ∆H° based on the structure of the conjugate bases. [Assume T = 298 K.] (a)303views
Textbook QuestionCalculate ∆G°, ∆H°, and ∆S° for the following acid–base reactions. Rationalize the value of ∆H° based on the structure of the conjugate bases. [Assume T = 298 K.] (c)305views
Textbook QuestionWrite the rate law for the following reaction and identify which molecules are present in the rate-determining step. Draw a possible transition state and propose a mechanism.302views
Textbook QuestionFor the following values of ∆H° , ∆S°, and T, tell whether the process would be favored. (a) ∆H° = -15 kcal/mol ; ∆S° = +37 cal/mol•K ; T = 273 K413views
Textbook Question(•) For each of the following acid–base reactions, (iii) calculate ∆G° If a pKₐ is not one of the ten common ones we learned in Chapter 4, it will be given to you. (a)316views
Textbook QuestionWhen ethyl bromide is added to potassium tert-butoxide, the product is ethyl tert-butyl ether. CH3CH2—Br + (CH3)3C—O- K+ —> (CH3)3C—O—CH2CH3 ethyl bromide potassium tert-butoxide ethyl tert-butyl ether a. What happens to the reaction rate if the concentration of ethyl bromide is doubled?316views
Textbook QuestionWhen ethyl bromide is added to potassium tert-butoxide, the product is ethyl tert-butyl ether. CH3CH2—Br + (CH3)3C—O- K+ —> (CH3)3C—O—CH2CH3 ethyl bromide potassium tert-butoxide ethyl tert-butyl ether b. What happens to the rate if the concentration of potassium tert-butoxide is tripled and the concentration of ethyl bromide is doubled? c. What happens to the rate if the temperature is raised?649views
Textbook QuestionUsing the bond-dissociation energies in Table 5.6 (see Section 5.3.1), estimate the equilibrium constant of the following reaction at 298 K.<IMAGE>336views
Textbook QuestionFor the following reactions we have not seen yet, which side, if either, would be favored by increasing the temperature? (c) ⇌342views
Textbook QuestionFor the following reactions we have not seen yet, which side, if either, would be favored by increasing the temperature? (d) ⇌344views
Textbook QuestionFor the following equilibrium processes and the corresponding ∆G° , calculate (i) K_eq and (ii) the % composition of the equilibrium mixture (% reactants, % products) at 298 K.(a) <IMAGE>308views
Textbook QuestionFor the following equilibrium processes and the corresponding ∆G° , calculate (i) K_eq and (ii) the % composition of the equilibrium mixture (% reactants, % products) at 298 K.(b) <IMAGE>357views
Textbook QuestionFor each pair of reactions, predict which will happen more quickly.[For (a) and (b), think about the stability of the bases involved.](a) <IMAGE>329views
Textbook QuestionFor the following equilibrium processes and the corresponding ∆G° , indicate whether you expect the equilibrium constant to be greater than, equal to, or less than 1. Justify your expectation in words.(b) <IMAGE>302views
Textbook QuestionFor the following acid–base reactions studied in Assessment 5.25, draw a likely transition state. Be sure to indicate in your drawing the degree to which bonds are broken or formed.(a) <IMAGE>333views
Textbook QuestionFor the following acid–base reactions studied in Assessment 5.25, draw a likely transition state. Be sure to indicate in your drawing the degree to which bonds are broken or formed.(c) <IMAGE>275views
Textbook QuestionFor the following acid–base reactions studied in Assessment 5.25, draw a likely transition state. Be sure to indicate in your drawing the degree to which bonds are broken or formed.(b) <IMAGE>329views
Textbook Questiond. Calculate ∆G° for the conversion of “axial” methylcyclohexane to “equatorial” methylcyclohexaneat 25 °C.359views
Textbook Questiona. Calculate the percentage of isopropylcyclohexane molecules that have the isopropyl substituent in anequatorial position at equilibrium. (Its ∆G° value at 25 °C is -2.1 kcal/mol.)348views
Textbook QuestionThe relative rate of reaction for the cis alkene (E) is given in Table 22.2. What do you expect the relative rate of reaction for the trans alkene to be?313views
Textbook QuestionExplain why the half-life (the time it takes for one-half of the compound to be metabolized) of Xylocaine is longer than that of Novocaine.322views
Textbook QuestionIn a reaction in which reactant A is in equilibrium with product B at 25 °C, what relative amounts of A and B are present at equilibrium if ∆G° at 25 °C isa. 2.72 kcal/mol?b. 0.65 kcal/mol?259views
Textbook QuestionIn a reaction in which reactant A is in equilibrium with product B at 25 °C, what relative amounts of A and B are present at equilibrium if ∆G° at 25 °C isc. -2.72 kcal/mol?d. -0.65 kcal/mol?301views
Textbook QuestionThe reaction of chloromethane with hydroxide ion at 30°C has a ΔG° value of −21.7 kcal/mol. What is the equilibrium constant for the reaction?258views
Textbook QuestionWhich of the following parameters would be different for a reaction carried out in the presence of a catalyst compared with the same reaction carried out in the absence of a catalyst?∆G°, ∆H‡, Ea, ∆S‡, ∆H°, Keq, ∆G‡, ∆S°, k307views
Textbook QuestionUnder base-catalyzed conditions, two molecules of acetone can condense to form diacetone alcohol. At room temperature (25 °C), about 5% of the acetone is converted to diacetone alcohol. Determine the value of ΔG° for this reaction.Acetone <IMAGE> + OH- ⇌ diacetone alcohol <IMAGE> 340views
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