Question B2: Kinetics of a reversible, first-order reactionThe acid-catalysed conversion of y-hydroxybutyric acid (GHBA) into its lactone, y-butyrolactone (GBL) is areversible reaction. The GHBA to GBL forward reaction is first-order with respect to the GHBAconcentration; the GBL to GHBA reverse reaction is first-order with respect to the GBL concentration.Time/minGBLAn experimental study of the kinetics of this reaction was undertaken in 0.2 mol L¹ hydrochloric acid (HCI) at298 K. The initial concentration of GHBA was 18.23 x 10³ mol L¹. The concentration of GBL in solution wasfollowed as a function of time (t), as indicated in Table B.3.concentration/10³ mol L¹00212.41363.73504.96656.10807.081008.11Table B.3: Experimental data corresponding to the GHBA to GBL conversion.LC13.285Use the data in Table B.3 to determine the equilibrium constant and the first-order rate constants for bothforward and reverse reactions. 15:44But how good is this approximation for reactive intermediates in the Earth's atmosphere?Let us consider the Earth's atmosphere at an altitude of 80 km above the Earth's surface, where thetemperature is "200 K.Here the combined concentration, [M], of nitrogen gas (N₂) and molecular oxygen (0₂) is3 x 10¹ molecules cm³, with [M] = [N₂] + [0₂]: molecular oxygen comprises around 20% of this.Molecular oxygen (O₂) at these altitudes can be photochemically decomposed to excited oxygen atoms, o(often reported as O('D) and ground-state oxygen atoms,O (often reported as O(³P):O₂+ hv0+0(A.1)In this reaction hv represents a photon of light of sufficient energy to cause the decomposition of O₂. Therate of this reaction can be represented as labsThe major loss processes for these atoms are:andX0'+M²0+M(A.2)k₂= 1.4x10-33 cm molecule-2 s-10+0₂ + M²0₂ + M(A.3)In reactions (A.2) and (A.3), M = N₂ or O₂, with k, being the second-order rate constant for reaction (A.2),and k, being the third-order rate constant for equation (A.3). At the altitude and temperature considered,these composite rate constants have the following values.kg = 3x10-11 cm³ molecule-1 s-1

Reversible reaction:- γ-hydroxybutyric acid (GHBA) ⇄K2K1 γ-butyrolactone (GBL)K1=K2 = 1st order…

An experimental study of the kinetics of this reaction was undertaken in 0.2 mol L¹ hydrochloric acid (HCI) at 298 K. The initial concentration of GHBA was 18.23 x 10³ mol L¹. The concentration of GBL in solution was followed as a function of time (t), as indicated in Table B.3. Time/min GBL concentration /10³ mol L¹ 0 0 21 2.41 36 3.73 50 4.96 65 6.10 80 7.08 100 8.11 Table B.3: Experimental data corresponding to the GHBA to GBL conversion. 13.28 Use the data in Table B.3 to determine the equilibrium constant and the first-order rate constants for both forward and reverse reactions.

An experimental study of the kinetics of this reaction was undertaken in 0.2 mol L¹ hydrochloric acid (HCI) at 298 K. The initial concentration of GHBA was 18.23 x 10³ mol L¹. The concentration of GBL in solution was followed as a function of time (t), as indicated in Table B.3. Time/min GBL concentration /10³ mol L¹ 0 0 21 2.41 36 3.73 50 4.96 65 6.10 80 7.08 100 8.11 Table B.3: Experimental data corresponding to the GHBA to GBL conversion. 13.28 Use the data in Table B.3 to determine the equilibrium constant and the first-order rate constants for both forward and reverse reactions.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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