A reaction is made up in the following way: 13 mL of 4.1M acetone + 13 mL of 1.8 M HCI + 12 mL of 0.0057 M I2 + 13 mL of water. It takes 352 seconds for the l2 color to disappear from the reaction mixture. What was the rate of reaction? Express you answer as a decimal number (no exponents). Include proper (abbreviated) units. Your Answer:

A reaction is made up in the following way: 13 mL of 4.1M acetone + 13 mL of 1.8 M HCI + 12 mL of 0.0057 M I2 + 13 mL of water. It takes 352 seconds for the l2 color to disappear from the reaction mixture. What was the rate of reaction? Express you answer as a decimal number (no exponents). Include proper (abbreviated) units. Your Answer:

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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2. The decomposition reaction of HO2 is given by 4 HO, (g) → 2 H2O (g) + 3 O, (g). From the following kinetics data (concentration of HOz vs. time) and two figures below, answer the following questions. Time (min) [HO;] M (or mol/L) 0.0000 2.0000 1.2500 0.66667 0.5 2.5000 0.40000 3.7500 0.28571 In [ HO, ] 1 5.0000 0.22222 [ HO, 1 4.5 2. The reaction order of HO2 should -1 be order. 1.5 a) Zero-th b) First c) Second time (min) time (min) d) None of the above
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5.00 mL 4.50 M acetone + 10.0 mL 1.15 M HCl + 10.0 mL 0.00200 M I2 + 25.0 mL H2O A student found that it took 146 seconds for the color of the I to disappear. a. What was the rate of the reaction? Hint: First find the initial concentration of Iz in the reaction mixture, [I2]o. Then use the equation Rate At t M/s b. Write the rate equation. (Abbreviate acetone to ace, H* ion to H", and iodine to I2. Represent the order of reaction with respect to acetone as m, the order of reaction with respect to iodine as n, and the order of reaction with respect to H* as p). c. Select all the unknown variables in the equation in part (b). Rate O[Ace] (Previous Next
Consider this reaction: NH₂OH(aq) →NH3(aq) + H₂O (aq) At a certain temperature it obeys this rate law. -1 -1 rate -(0.00284 M¹¹) [NH₂OH]² Suppose a vessel contains NH₂OH at a concentration of 1.33M. Calculate the concentration of NH₂Oн in the vessel 840. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Another common component of reaction mechanism is a catalyst. These are compounds that change the reaction mechanism and provide a pathway with a lower activation energy, and correspondingly faster reaction rate. They are a reactant in an early step in the mechanism and a product in a later step. They do not appear in the overall reaction but do appear in the rate law. 3. A reaction occurs by the following mechanism; Step 1 Ce4+ + Mn²+ →→ Ce³+ + Mn³+ Step 2 Ce4+ + Mn³+ → Ce³+ + Mn²+ Step 3 Tit+ Mn+→ Ti³+ + Mn²+ a. Write the overall reaction. b. Identify each of the components as a reactant, product, intermediate, or catalyst; Mn²+ Mn³+ Ce4+ Ce ³+ Mn4+ Tit Ti³+ C. Assuming that the catalyst is involved in the rate determining step, what is the rate law for this reaction? 4. Under certain conditions, the reaction: 2 NO + Cl₂ → 2 NOCI is found to be second order in NO and first order Cl₂. Given the following mechanism; Step 1 NO + Cl2 → NOCI₂ Step 2 NOCI₂ + NO 2 NOCI a. What are the…