Answered: 13 Write and name the other product of…

13 Write and name the other product of each of the following reactions: Acid catalyst C4H9OH H2O (Concentrated Sulphuric acid) Acid catalyst C3H7OH H2O (Concentraled Sulphuric acid)

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 9RQ: What characterizes an electrolytic cell? What is an ampere? When the current applied to an...

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The peroxydisulfate ion (S2O8-2) reacts with the iodide ion in aqueous solution via the reaction: S2O82-(aq) + 3I- → 2SO4(aq)+ I3-(aq). An aqueous solution containing 0.050 M of S2O8-2 ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. Time (s) 0.00 400.0 800.0 1200.0 1600.0 [I‑] (M) 0.072 0.057 0.046 0.037 0.029 Determine the average rate of disappearance of I- between 400.0 s and 800.0 s in M/s. Determine the average rate of disappearance of I- in the initial 400.0 s in M/s. Determine the average rate of disappearance of I- between 1200.0 s and 1600.0 s in M/s. Determine the concentration of S2O82- remaining at 400 s in M. Determine the concentration of S2O82- remaining at 800 s in M. Determine the concentration of S2O82- remaining at 1600 s in M.
The peroxydisulfate ion (S2O8-2) reacts with the iodide ion in aqueous solution via the reaction: S2O82-(aq) + 3I- → 2SO4(aq)+ I3-(aq). An aqueous solution containing 0.050 M of S2O8-2 ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. Time (s) 0.00 400.0 800.0 1200.0 1600.0 [I‑] (M) 0.072 0.057 0.046 0.037 0.029 Determine the concentration of S2O82- remaining at 400 s in M. Determine the concentration of S2O82- remaining at 800 s in M. Determine the concentration of S2O82- remaining at 1600 s in M.
8 Reactions between certain organic (alkyl) halides and water produce alcohols. Consider the overall reaction for t-butyl bromide (2-bromo-2-methylpropane). (CH3)3CBr(aq) + H2O(1) →(CH3)3COH(aq) + H*(aq) + Br "(ag) k[(CH3)3CB1]. The accepted mechanism for the The experimental rate law is rate = %3D reaction is shown below. (1) (CH3)3C-Br(aq) →(CH3)3C*(aq) + Br "(aq) [slow] (2) (CH3)3C*(aq) + H2O(1) →(CH3)3C-OH2*(aq) [fast] (3) (CH3)3C-OH2*(aq) →H*(aq) + (CH3)3C-OH(aq) [fast] a) Why doesn't H2O appear in the rate law? b) Write rate laws for the elementary steps. c) What intermediates appear in the mechanism? d) Show that the mechanism is consistent with the experimental rate law. ed to the of consumption of N
34. A key step in the formation of sulfuric acid from dissolved SO2 in acid precipitation is the oxidation of hydrogen sulfite ion by hydrogen peroxide: HSO, (ag) + H2 O2 (aq) → HSO, (aq) + H2O(t) The mechanism involves peroxymonosulfurous acid, SO20OH¯: k1 HSO, (aq) + H2 O2 (ag) 2 SO200H (ag) + H2 O (l) k-1 k2 SO200H (aq) + H3O+ (aq) → HSO, (ag) + H3O† (aq) By making a steady-state approximation for the reactive intermediate concentration, [SO20OH (ag)], express the rate of formation of HSO, (aq) in terms of the concentrations of HSO, (aq), H2O2 (aq), and H3 O“(aq).
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