In this experiment you studied the following net chemical reaction that we will call reaction (1): H,0, + 2 H* + 21 -1, + 2 H,0 (1) with the following proposed three-step reaction mechanism: H,0, + - OH" + HOI OH + H* - H,0 Step 1: (slow) Step 2: (very fast) Step 3: (fast) HOI + H* + -2 + H20 In neutral solution containing only hydrogen peroxide and iodide ion, a different net chemical reaction occurs: 2 H,0, - 2 H,0 + 0,(g) (2) The following three-step reaction mechanism has been proposed to explain reaction (2): H,0, +1 - OH + HOI Step 2a: (very fast) OH + HOI - 10 + H,0 Step 1: (slow) H20, + 10 I + H20 + 0,(g) 2 HA0 - 2 H0t O Show that when you sum the three reaction steps the net result is reaction (2): Step 3a: (fast)

In this experiment you studied the following net chemical reaction that we will call reaction (1): H,0, + 2 H* + 21 -1, + 2 H,0 (1) with the following proposed three-step reaction mechanism: H,0, + - OH" + HOI OH + H* - H,0 Step 1: (slow) Step 2: (very fast) Step 3: (fast) HOI + H* + -2 + H20 In neutral solution containing only hydrogen peroxide and iodide ion, a different net chemical reaction occurs: 2 H,0, - 2 H,0 + 0,(g) (2) The following three-step reaction mechanism has been proposed to explain reaction (2): H,0, +1 - OH + HOI Step 2a: (very fast) OH + HOI - 10 + H,0 Step 1: (slow) H20, + 10 I + H20 + 0,(g) 2 HA0 - 2 H0t O Show that when you sum the three reaction steps the net result is reaction (2): Step 3a: (fast)

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section: Chapter Questions

Problem 90IL: The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common...

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The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
In this experiment you studied the following net chemical reaction that we will call reaction (1): H,0, + 2 H* + 21 - 1, + 2 H,0 (1) with the following proposed three-step reaction mechanism: Step 1: (slow) H,0, +1 - OH + HOI Step 2: (very fast) OH + H* - H,0 Step 3: (fast) HOI + H* + - 2 + H,0 In neutral solution containing only hydrogen peroxide and iodide ion, a different net chemical reaction occurs: 2 H,0, - 2 H,0 + 0,(g) (2) The following three-step reaction mechanism has been proposed to explain reaction (2): Step 1: (slow) H20, +1 - OH + HOI Step 2a: (very fast) OH + HOI -- 10- + H,0 H,0, + 10 -I + H20 + 0,(g) 2 H2 02 → 2 HzO + OLCJ) Show that when you sum the three reaction steps the net result is reaction (2): Step 3a: (fast) What would be the expected rate law for the reaction mechanism, assuming that the rate of reaction (2) is limited by the slow Step 1? Is the expected rate law for reaction (2) the same as or different from the rate law you determined for reaction (1)?
In this experiment you studied the following net chemical reaction that we will call reaction (1): H,0, + 2H + 21 - 1, + 2 H,0 (1) with the following proposed three-step reaction mechanism: H,0, +1 - OH + HOI OH + H* - H,0 HOI + H* + - l + H,0 Step 1: (slow) Step 2: (very fast) Step 3: (fast) In neutral solution containing only hydrogen peroxide and iodide ion, a different net chemical reaction occurs: 2 H,02 - 2 H,0 + 0,{g) (2) The following three-step reaction mechanism has been proposed to explain reaction (2): Step 1: (slow) H,0, +1 - OH + HOI Step 2a: (very fast) OH + HOI 10 + H,0 H,0, + 10I + H20 + 0,(g) 2 H202 → 2 HzO + OeC5) Show that when you sum the three reaction steps the net result is reaction (2): Step 3a: (fast) What would be the expected rate law for the reaction mechanism, assuming that the rate of reaction (2) is limited by the slow Step 1?
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Grade 12 solution
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