### Understanding Reaction Mechanisms and Rate LawsIn chemical kinetics, understanding the mechanisms and deriving the rate laws of reactions is crucial to predict how different factors influence reaction rates. Below, we explore the rate laws for two different proposed mechanisms for a reaction involving hydrogen (H₂) and bromine (Br₂) to produce hydrogen bromide (HBr).#### Mechanism II:$$H_2 + Br_2 \xrightarrow{k_2} 2HBr \hspace{5pt} (\text{slow})$$### Exercises**a) Derive the rate law for Mechanism I.***Show all work on paper - use a ^ here to indicate a superscript if necessary.*\[ \boxed{\text{Answer}} \]**b) Derive the rate law for Mechanism II.***Show all work on paper - use a ^ here to indicate a superscript if necessary.*\[ \boxed{\text{Answer}} \]**c) The observed rate law for the reaction is $r = k_{obs}[H_2][Br_2]^{1/2}$. Which mechanism is consistent with this observation? Clearly indicate Mechanism I or Mechanism II.**\[ \boxed{\text{Answer}} \]**d) Based on your answer to part (c) above, write the observed rate constant $k_{obs}$ in terms of the rate constants used in the relevant mechanism.***Show all work on paper - use a ^ here to indicate a superscript if necessary.*\[ \boxed{\text{Answer}} \]### Detailed Explanation of Mechanisms and Graphs/DiagramsThere is no graphical or diagrammatic representation in the image. However, you are requested to derive and analyze the rate laws and mechanisms as described above. Remember to provide detailed steps in your derivations and clearly indicate any assumptions or approximations you make.These exercises are designed to help you understand how different mechanistic steps impact the overall rate law of the reaction and the importance of intermediates in determining reaction kinetics. In-depth knowledge of these aspects is essential for students aiming to master the principles of chemical kinetics. ### Reaction Mechanisms for the Formation of HBrIn addition to filling in the blanks below, show all of your work for this problem on paper for later upload.#### Mechanism I:Two mechanisms have been proposed for the formation of HBr from elemental hydrogen and bromine. Here is Mechanism I:\[ \text{Br}_2 + \text{M} \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2 \text{Br} + \text{M} \quad(\text{fast})\]\[ \text{Br} + \text{H}_2 \stackrel{k_2}{\rightarrow} \text{HBr} + \text{H} \quad(\text{slow})\]\[ \text{H} + \text{Br}_2 \stackrel{k_3}{\rightarrow} \text{HBr} + \text{Br} \quad(\text{fast})\]where M is called an inert, third-body intermediate (for example, $ \text{N}_2 $).#### Mechanism II:Mechanism II is:\[ \text{H}_2 + \text{Br}_2 \stackrel{k_2}{\rightarrow} 2 \text{HBr} \quad(\text{slow})\]### Questions:a) Derive the rate law for Mechanism I (show all work on paper - use a ^ here to indicate a superscript if necessary).\[ \boxed{\phantom{Rate\ Law\ Here}} \]b) Derive the rate law for Mechanism II (show all work on paper - use a ^ here to indicate a superscript if necessary).\[ \boxed{\phantom{Rate\ Law\ Here}} \]Please ensure to document each step carefully and write legibly for your submission.

Rate of reaction is defined as the rate at which products are formed or reactants are consumed. Rate…

In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. Two mechanisms have been proposed for the formation of HBr from elemental hydrogen and bromine. Here is Mechanism I: Br2 + M 2 2 Br + M fast Br + H2 4 HBr + H slow H + Brz 4 HBr + Br fast where M is called an inert, third body intermediate (for example, N2). Mechanism II is: H + Brz 2 HBr (slow) a) Derive the rate law for Mechanism I (show all work on paper - use a ^ here to indicate a superscript if necessary). b) Derive the rate law for Mechanism II (show all work on paper - use a ^ here to indicate a superscript if necessary).

In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. Two mechanisms have been proposed for the formation of HBr from elemental hydrogen and bromine. Here is Mechanism I: Br2 + M 2 2 Br + M fast Br + H2 4 HBr + H slow H + Brz 4 HBr + Br fast where M is called an inert, third body intermediate (for example, N2). Mechanism II is: H + Brz 2 HBr (slow) a) Derive the rate law for Mechanism I (show all work on paper - use a ^ here to indicate a superscript if necessary). b) Derive the rate law for Mechanism II (show all work on paper - use a ^ here to indicate a superscript if necessary).

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...

See similar textbooks

Similar questions

16) The reaction (C2H5)2(NH2) + 12 (C2H5)2(N2) + 2HI gives the following data. Expt Initial(C2H5)2(NH2) mol L-1 Initial 12 mol L-1 Initial rate of formation of (C2H5)2(N2) mol L-1min-1 1 0.015 0.015 3.15 x 10-1 2 0.015 0.045 9.45x 10-1 3 0.030 0.045 18.9 x 10-1 a) Determine the order of the reaction with respect to each reactant. Explain how you arrived at each answer. (Show your method) b) What is the overall order of the reaction? c) Write the rate law expression. d) Calculate the rate constant, k and provide the proper units. e) If (C2H5)2(N2) is formed at a rate of 9.45 M/s in experiment 3, what is the rate of appearance of HI? f) In experiment 3, assuming it goes to completion, if all of [(C2H5)2(NH2) ] is reacted, what would be the amount of 12 remaining?
Please provide proper explanation of the concept and solution
Consider the following reaction mechanism. Step 1 : W2 ⇌ 2W (fast) Step 2 : W + Z ⇌ D + F (fast) Step 3 : W + F → M (slow)Write the predicted rate law
Parts A - D.
Analyze the following reaction mechanism: 1. Н-О2 H20 + O 2. O + CF2CI2 3. CIO + Oз — CІ + 202 4. CI + CF2CI –→ CF2CI2 → CIOÓ + CF2CI Based on the reaction mechanism, what is the molecularity of elementary step 1? A) unimolecular B) bimolecular C) termolecular D) quadrimolecular
Consider the mechanism: NO2(8) + SO2(g) → NO(g) + SO3(g) NO(g) + ½ O2(g) –→ NO2(g)
For a simple reaction, S 1 P, k1 is the rate of the forward reaction and k-1 is the rate of the backwards reaction. The k1 in the absence of any enzyme was 0.01/s. The k1 in the presence of enzyme was 5,000,000/s. Calculate the rate enhancement (k1 catalyzed divided by k1 uncatalyzed) provided by the enzyme. If the equilibrium constant in the absence of enzyme is 1 x 104, what is the equilibrium constant (Keq) in the presence of enzyme?
LINEZOLID (600 MG TAB, t1/2 = 7 hours) COMPUTED REACTION CONSTANT BASED ON HALF LIFE: Assuming a first order reaction, 0.693 k t = 1/2 7 hrs, = 0.693 k 0.693 7 hrs. k = 0.099 k = hr. k 9.9 X 10 -2 1 hr. HOW MANY HOURS WILL IT TAKE TO ELIMINATE 73% OF THE DRUG AFTER THE INITIAL DOSE SHOW YOUR COMPUTATION AND HALF-LIFE GRAPH
Write the rates for the following reactions in terms of the disappearance ofreactants and appearance of products: a. 3 O2 → 2 O3b. C2H6 → C2H4 + H2c. ClO- + Br- + → BrO- + Cl d. (CH3)3CCl + H2O → (CH3)3COH+ H+ Cl- e. 2 AsH3 → 2 As + 3 H2
Consider the overall reaction 2A + B ⇌ 2C(g) with proposed mechanism for this reaction: A + B ⇌ C + D (slow) A+D ⇌ C (fast)What is the rate law for this proposed mechanism?
ST6C.3 - Radioactive iodine-131 decays with first-order kinetics (like all radioactive material) and has a half-life of 8 days. What percent of the original sample is left after. 32 days? 50% 8 days? 25% 64 days? 0.78% 12.5% 16 days? 1.56% 0.39% 6.25% 3.13%
The rate constant for the reaction of nitrogen with oxygen was determined at four temperatures. N2(g) + O2(g) T(K) 2NO(g) k (cm3/molecule⚫s) 250 7.18 x 10-8 275 1.36 x 10-7 300 2.31 x 10-7 325 3.46 x 10-7 3rd attempt Part 1 (1 point) Plot these data to calculate the activation energy of the reaction. kJ/mol Part 2 (1 point) Plot these data to calculate the frequency factor A for the reaction. cm3/molecules