6.16Before solving the problem please also give a brief explanation of the concept or associated equation(s) and variables. 6.16 The reaction mechanismA2 A+A (fast)A+B P (slow)involves an intermediate A. Deduce the rate law for the for-mation of P.

Reaction Mechanism and Rate Law: A reaction mechanism provides a detailed sequence of steps by which…

Answered: 6.16 The reaction mechanism A2 A+A…

6.16 The reaction mechanism A2 A+A (fast) A+B P (slow) involves an intermediate A. Deduce the rate law for the for- mation of P.

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter7: Reaction Rates And Chemical Equilibrium

Section: Chapter Questions

Problem 7.14P

See similar textbooks

Similar questions

(5) IV. Hydrogen and carbon monoxide react to give formaldehyde under certain conditions. H2(g) + CO(g) = HCHO(g) The mechanism proposed for this reaction is H2(g) = 2 H(g) H(g) + CO(g) H(g),+ HCO(g) → HCHO What rate law is derived from this mechanism? Step 1 Step 2 Step 3 fast HCO(g) slow > fast
The reaction H2O + SO3 → H2SO4 is a source of acid rain in Earth’s atmosphere. It is thought to occur via the two-step mechanism shown at the right. (1) H2O+SO3 -->H2OSO3 (2) H2O+H2OSO3-->H2O+H2SO4 a. What is the experimental rate law for the overall reaction if step (1) is the rate determining step? b. What is the experimental rate law for the overall reaction if step (2) is the rate determining step?
11. (8 pt) Enrofloxacin is a drug used for dogs and cats to combat bacterial infections.A dog was given an intramuscular injection of enrofloxacin, and just after the injection, the initial concentration of the drug in the dog’s blood was 5.8Í10–6 M. If the enrofloxacin disappears in a first-order process with a half-life of 4.6 hours, how many hours will it take for the enrofloxacin concentration of drop to one-eighth (1/8th) of the initial concentration (i.e., 0.125[A]0)?
A suggested mechanism for the decomposition of peroxide (H2O2) is H2O2(aq) ->>> 2OH(aq) H2O2(aq) + OH(aq) H2O()+ HO2(g) HO2(g) + OH(aq)) → H2O(l) + O2 (g) ->> Based on the mechanism which statement is true? (1) The rate law is rate = k[H202] (2) the molecularity of the slow reaction is 4 (4) OH2 is an intermediate (3) OH is a catalyst A Moving to the next question prevents changes to this answer. MacBook Pro fast slow fast
G.130.
A mechanism involving the following elementary reactions has been proposed: 2 X (g) → X2 (g) (fast) X2 (g) +Y(g) = XY(g)+X(g) (slow) (8a) What is the reaction intermediate in this mechanism? (8b) What overall rate law will this mechanism produce?
Be sure to answer all parts. The reaction between NO2 and CO to produce NO and CO2 is thought to occur in two steps: (k1)Step 1: NO2 + NO2 ----> NO + NO3 (k2)Step 2: NO3 + CO ---->NO2 + CO2 The experimental rate law is rate = k[NO2]2. (a) Write the equation for the overall reaction. Do not include phase abbreviations. (b) Identify the intermediate(s). (c) Identify the rate-determining step.
The proposed 3-step mechanism for a reaction isStep 1) X(g) + Y(g) A(g) fast, reaches equilibrium (For Step 1, k1 = forward rate constant & k-1 = reverse rate constant.)Step 2) A(g) + Z(g) B(g) slow (k2 = rate constant) Step 3) B(g) P(g) fast (k3 = rate constant) a) What is the overall reaction? b) What is the rate law supported by this mechanism? Explain your answer. c) The following is experimental data found for this reaction: Initial [X] (M) Initial [Y] (M) Initial [Z] (M) Initial Rate (M/day) Exp 1 0.150 0.150 0.150 0.569 Exp 2 0.250 0.150 0.150 0.948 Exp 3 0.250 0.300 0.150 3.793 Exp 4 0.300 0.350 0.200 6.196 i) What is the experimentally determined rate law? ii) Determine the rate constant and include units. d) Does your experimentally determined rate law support the proposed mechanism? Explain your answer. e) ΔΔHo = -347 kJ/mol for the overall reaction. Draw a reasonable reaction profile for the proposed mechanism.…
(Q88) A first-order reaction has a half-life of 16.9 seconds. How long (in seconds) will it take for the concentration of the reactant in the reaction to fall to one-eighth of its initial value? (3 sf)
(7pts) The rate law for the reaction 3A C is Rate = 0.951 M' hr1 [A]? What is the half-life for the reaction if the initial concentration of A is 0.750 M? How long will it take for the concentration to be reduced to 0.050 M?
(Q79) Using the information provided, what are the reaction orders for CHCI3 and Cl2 respectively? CHCI3 (g) + Cl2 (g) --> CCI4 (g) + HCI (g) [CHCI3] (M) [Cl2] (M) Initial Rate (M/s) 0.010 0.010 0.0035 0.020 0.010 0.0069 0.020 0.020 0.0098 0.040 0.040 0.027 1 and 0.5 O 1 and 1 O 2 and 1 O 0.5 and 0.5 O 0.5 and 1
(Q80) Using the information provided (and your work from Q79), what is the numerical value of the rate constant for the rate law determined in Q79? CHCI3 (g) + Cl2 (g) --> CCI4 (g) + HCI (g) [CHCI3] (M) [C2] (M) Initial Rate (M/s) 0.010 0.010 0.0035 0.020 0.010 0.0069 0.020 0.020 0.0098 0.040 0.040 0.027