The answers can be found at the end of the practice problem set, and full solutions can be discussed during tutorial time and/or office hours. 1. Ethanol (EtOH) reacts with H* and Cl to give ethyl chloride (EtCI). A possible mechanism is shown below. The first step is thought to be reversible, with rate constant k.1 corresponding to the reverse of step 1. The second step is assumed to be irreversible. Step 1: ETOH + H* 3 ETOH,+ Reverse of Step 1: EtO H,+ Et0H + H+ Step 2: EtOH,+ + Cl- 3 EtCl + H20 a) What is the overall balanced chemical equation? b) What is/are the reaction intermediate(s)? c) Using the steady state approximation, derive the general rate law for this mechanism. d) What does the general rate law simplify to if we assume step 2 is the rate determining step? 2. A chemical reaction increases in rate by a factor of 12.9 when the temperature is raised from 5.0°C to 30.0°C (all other conditions such as concentrations remain the same). Calculate the activation energy (in kJ mol-1) for this reaction. 3. What are appropriate units for the rate constant for the hypothetical rate law: rate = k[A]²[B][C]?

The answers can be found at the end of the practice problem set, and full solutions can be discussed during tutorial time and/or office hours. 1. Ethanol (EtOH) reacts with H* and Cl to give ethyl chloride (EtCI). A possible mechanism is shown below. The first step is thought to be reversible, with rate constant k.1 corresponding to the reverse of step 1. The second step is assumed to be irreversible. Step 1: ETOH + H* 3 ETOH,+ Reverse of Step 1: EtO H,+ Et0H + H+ Step 2: EtOH,+ + Cl- 3 EtCl + H20 a) What is the overall balanced chemical equation? b) What is/are the reaction intermediate(s)? c) Using the steady state approximation, derive the general rate law for this mechanism. d) What does the general rate law simplify to if we assume step 2 is the rate determining step? 2. A chemical reaction increases in rate by a factor of 12.9 when the temperature is raised from 5.0°C to 30.0°C (all other conditions such as concentrations remain the same). Calculate the activation energy (in kJ mol-1) for this reaction. 3. What are appropriate units for the rate constant for the hypothetical rate law: rate = k[A]²[B][C]?

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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Explain your reasoning, please. Thank you.