The answer of the question is in the picture
Below is a mechanism for the reaction A+B- P 5. 2A ? A+C rate constant kl...
The reaction 2A + B → C occurs by the following 2 step mechanism: A + B ------(k1)------> AB AB ------(-k1) ------> A+B AB + A ----- (k2)------> C Apply the steady-state approximation for the reaction intermediate concentration to obtain the overall rate law from this mechanism: a) k1 [A][B] b) k1k2[A][B]/((-k1) - k2[A]) c) k1k2[A]^2[B]/((-k1)+k2[A])
2.4 Using the steady state approximation derive the rate expression for the formation of C in the reaction 2A + B (g) → 2C(9) on the basis of the following proposed mechanism ki ZA K-1 X + B K2 20 To what expression does the rate expression reduce if the second reaction is slow, the initial equilibrium established very rapidly. (8)
4. The mechanism suggested for the reaction, 2 A + B +20 A+ AL I + B + 2C forward rate constant kı, backward rate constant k., constant k2 The rate law obtained on applying the steady state approximation is, A) Rate = kika[A] [B] B) Rate = kik[A] [B]/(k.1 + 2[B]) C) Rate = kık[A][B] D) Rate = kik[A]?/(k.1 +k2[B]) E) Rate = kika[A] [B]/(ki + k2[B])
A chemical reaction, A+B → P, has the following mechanism: 2A< Ki>A, (fast to equilibrium) A+B&K, ™C (fast to equilibrium), A,+C-k>P+ 2A (slow) where Kį and K2 are the equilibrium constants for the first two reactions, respectively. k3 is the rate constant for the third reaction. (a) [5 points] Based on this mechanism, show that the rate of product (P) formation is: d[P] – k[A[B], where k is the rate constant of the overall reaction. Write k in terms of...
5) The reaction, 2A + B P (P is the product). proceeds via a rapid pre-equilibrium (with equilibrium constant, K) followed by a slow rate determining step (with rate constant, kz) as shown below: 2A к = Az (fast pre-equilibrium) A2+B Products (slow) Develop an expression for the rate of formation of products as a function of [A], [B], K, and kz 6) The reaction, A+B+C - P(P is the product) proceeds by the following mechanism. k, A+B=0 I+CP "T"...
a. Write the rate law for this reaction. b. Calculate the rate constant. c. At what rate does KI disappear if the initial concentrations are [KI] = 0.0450 M and [(NH4)2S2O8] = 0.120 M? d. At what rate does (NH4)2S2O8 disappear under the conditions given in part c? The powers of 10 in the last boxes are 10^-3 Some data for this reaction follows: Experiment INHA.SoJON) T [Kn Initial Rate of Appearance of KL CMU's) 0200 0100 4.76 x 10...
A reaction has the mechanism A + B X + B rightarrow P with rate constants k_1, k_-1, and kr. Assuming a steady state approximation for [X] is valid, write the rate law for d[P]/dt?
Consider the mechanism. Step 1: Step 2: Overall: 2A B B+C HD 2A+ C D equilibrium slow Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate = 1
step by step Rates of Non-elementary reactions Class Activity Consider the following mechanism: 2NO N202 k-1 NzOz + C12-2+2 NOCI a. What is the net reaction? b. Which of the above species is an intermediate? Why? c. Find the rate of the overall reaction using the steady-state approximation. d. Repeat part (c) using the rate-determining step method, assuming the first-step is fast and at equilibrium and the second step is slow. 2NO N,02 (ast,at equilibrium) k-1 N202 + Cl2-22 NOCI...
Consider the following mechanism. step 1 2A > B slow B+ C D fast step 2 overall: 2A+C D Determine the rate law for the overall reaction (where the overall rate constant is represented as k) rate=