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2.4 Using the steady state approximation derive the rate expression for the formation of C in the reaction 2A + B (g...
I want the answer by using steady-state approximation < thank u in advance I reaction for...
I
want the answer by using steady-state approximation < thank u in
advance
I reaction for the thermal decomposition of acetaldehyde is: CH3CHO ·→ CH4 + CO A sequence of elementary steps proposed to explain the decomposition is as follows CH3CHO CH3' +CH3CHO CH3 +CH3 Derive an expression for the overall rate of decomposition of CH3CHO. Example 2. Ethyl nitrate pyrolysis has the following mechanism CH3'+ C2HsONO2 What is the rate expression consistent with this mechanism?
Consider the reaction mechanism: k A+B= X k-1 X+A_K2C+D Using the steady-state approximation, show that an...
Consider the reaction mechanism: k A+B= X k-1 X+A_K2C+D Using the steady-state approximation, show that an effective rate equation for [C] is rate=d[C]/dt = -keff[A] [B]. What is keff in terms of ki, k-1, k2, [A], and [B]? A kzkz[A][B]/(k-1[B]+k2) B kık2[B]/(k-1[B]+k2) C kzkz/(k-1+k2[A]) D kık2/k-1 E ki
6. Use the steady state approximation to derive a rate law for d[D/dt with the following...
6. Use the steady state approximation to derive a rate law for d[D/dt with the following mechanism A+B +C Step 1) Step 2) 7. a) What is the rate law for the mechanism in question (6) if the second step is the rate-limiting step? b) Express the activation energy for the overall reaction in terms of the activation energies for each step in the mechanism from part (a)
A chemical reaction, A+B → P, has the following mechanism: 2A< Ki>A, (fast to equilibrium) A+B&K, ™C (fast to...
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...
Below is a mechanism for the reaction A+B- P 5. 2A ? A+C rate constant kl...
Below is a mechanism for the reaction A+B- P 5. 2A ? A+C rate constant kl AtC 2A rate constant k B+C Prate constant k2 In this mechanism, C is an intermediate. nd the steady state approximation if necessary, determine the rate law for the reaction. (B) Under what conditions does the rate law become first order in [AJ? (C) Under what conditions does the rate not depend on [B]?
5) The reaction, 2A + B P (P is the product). proceeds via a rapid pre-equilibrium...
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"...
The reaction 2A + B → C occurs by the following 2 step mechanism: A +...
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])
(a) i) Use the steady-state approximation to derive the expression below for the rate of a...
(a) i) Use the steady-state approximation to derive the expression below for the rate of a free radical polymerisation, –d[M]/dt = kp[M](kdf[I]/kt) ½ ii) Given kd = 1015.2, e ^–128 kJmol–1/RT s –1, and f = 0.7 for AIBN, kp = 107.906, e ^–35.70 kJ mol–1/RT M – 1 s –1 for butadiene, and the data below, what is kt for polymerisation of butadiene in this system? [Butadiene] (M) [AIBN] (M) Rate (M s–1 ) T (°C) 0.85 1.59 x...
S. A) Derive the rate expression for a reaction between A and B species in solution...
S. A) Derive the rate expression for a reaction between A and B species in solution using a model that includes the diffusion of A and B to form an intermediate complex AB (use a steady-state approximation for AB). B) What does this expression looks like if the reaction is diffusion controlled?
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 + 0 + M 0+03 2 02 Apply the steady-state approximation to the concentration of atomic oxygen, and derive t...
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 + 0 + M 0+03 2 02 Apply the steady-state approximation to the concentration of atomic oxygen, and derive the rate law for the decomposition of ozone (M stands for a molecule that can exchange kinetic energy with particles undergoing the chemical reaction.)
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 +...
I
want the answer by using steady-state approximation < thank u in
advance
I reaction for the thermal decomposition of acetaldehyde is: CH3CHO ·→ CH4 + CO A sequence of elementary steps proposed to explain the decomposition is as follows CH3CHO CH3' +CH3CHO CH3 +CH3 Derive an expression for the overall rate of decomposition of CH3CHO. Example 2. Ethyl nitrate pyrolysis has the following mechanism CH3'+ C2HsONO2 What is the rate expression consistent with this mechanism?
Consider the reaction mechanism: k A+B= X k-1 X+A_K2C+D Using the steady-state approximation, show that an effective rate equation for [C] is rate=d[C]/dt = -keff[A] [B]. What is keff in terms of ki, k-1, k2, [A], and [B]? A kzkz[A][B]/(k-1[B]+k2) B kık2[B]/(k-1[B]+k2) C kzkz/(k-1+k2[A]) D kık2/k-1 E ki
6. Use the steady state approximation to derive a rate law for d[D/dt with the following mechanism A+B +C Step 1) Step 2) 7. a) What is the rate law for the mechanism in question (6) if the second step is the rate-limiting step? b) Express the activation energy for the overall reaction in terms of the activation energies for each step in the mechanism from part (a)
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...
Below is a mechanism for the reaction A+B- P 5. 2A ? A+C rate constant kl AtC 2A rate constant k B+C Prate constant k2 In this mechanism, C is an intermediate. nd the steady state approximation if necessary, determine the rate law for the reaction. (B) Under what conditions does the rate law become first order in [AJ? (C) Under what conditions does the rate not depend on [B]?
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"...
S. A) Derive the rate expression for a reaction between A and B species in solution using a model that includes the diffusion of A and B to form an intermediate complex AB (use a steady-state approximation for AB). B) What does this expression looks like if the reaction is diffusion controlled?
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 + 0 + M 0+03 2 02 Apply the steady-state approximation to the concentration of atomic oxygen, and derive the rate law for the decomposition of ozone (M stands for a molecule that can exchange kinetic energy with particles undergoing the chemical reaction.)
12. The following mechanism is proposed for the decomposition of ozone (O3) to O2: 03 + M 02 +...
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