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5. (6 pts) Suppose a reaction has the following mechanism: AB B + CD Assuming steady-state...
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...
A reaction has the mechanism A + B X + B rightarrow P with rate constants...
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 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
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])
4. The mechanism suggested for the reaction, 2 A + B +20 A+ AL I +...
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])
2.4 Using the steady state approximation derive the rate expression for the formation of C in the reaction 2A + B (g...
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)
Consider the following reaction on acetone (CH3COCH3), the mechanism is believed to involve four elementary steps:...
Consider the following reaction on acetone (CH3COCH3), the mechanism is believed to involve four elementary steps: CH3COCH; 4+ CH3 + CH3CO CH3 + CH3COCH; CH4 + CH3COCH, CH;COCH2 _ky → CH3 + CH2CO CH3 + CH3COCH, ko > CH3COCZH (a) Write down an expression for the rate of disappearance of CH3COCHz. (3 marks) Assume kz >> k[CH3), apply the steady-state approximation and work out an expression for (CH3) in term of kį, kz, kz and ke. Show all of your...
k1f M Br2 Br Br M kir (1) + k2,f BrH2 HBr H k2,r (2) + + ka,f HBr Br HBr2 (3) + + Experimentally measured rate expressi...
k1f M Br2 Br Br M kir (1) + k2,f BrH2 HBr H k2,r (2) + + ka,f HBr Br HBr2 (3) + + Experimentally measured rate expression for [HBr] given as below: d [HBr] Aexp [H2] [Br2]1/2 [HBr] 1+ A2expBr2 dt Consider the above elementary reactions mechanism proposed by Bodenstein to explain their experimental findings of the reaction rate of HBr. Reactions 1 and 2 are bi-directional (forward and reverse) while reaction 3 is uni-directional (forward only) as written....
A2. Chemical Kinetics (20 marks) MBr2 Br Br M k1 |(1) k2. Br H2 HBr H k2,r (2) k3,f HBr2 HBr Br (3) + Experimentally me...
A2. Chemical Kinetics (20 marks) MBr2 Br Br M k1 |(1) k2. Br H2 HBr H k2,r (2) k3,f HBr2 HBr Br (3) + Experimentally measured rate expression for [HBr] given as below: d [HBr] A1exp[H2] [Br2]1/2 HBr 1+ A2exp TBr2 dt Consider the above elementary reactions mechanism proposed by Bodenstein to explain their experimental findings of the reaction rate of HBr. Reactions 1 and 2 are bi-directional (forward and reverse) while reaction 3 is uni-directional (forward only) as written....
— O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism Suppose the...
— O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism Suppose the formation of nitrosyl chloride proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + Cl2(9) ► NOCI (9) km 2 NOCI (9) + NO(g) → 2 NOCI (9) kz Suppose also k«k. That is, the first slower than the second 0-0 Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical...
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...
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 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
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])
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)
Consider the following reaction on acetone (CH3COCH3), the mechanism is believed to involve four elementary steps: CH3COCH; 4+ CH3 + CH3CO CH3 + CH3COCH; CH4 + CH3COCH, CH;COCH2 _ky → CH3 + CH2CO CH3 + CH3COCH, ko > CH3COCZH (a) Write down an expression for the rate of disappearance of CH3COCHz. (3 marks) Assume kz >> k[CH3), apply the steady-state approximation and work out an expression for (CH3) in term of kį, kz, kz and ke. Show all of your...
k1f M Br2 Br Br M kir (1) + k2,f BrH2 HBr H k2,r (2) + + ka,f HBr Br HBr2 (3) + + Experimentally measured rate expression for [HBr] given as below: d [HBr] Aexp [H2] [Br2]1/2 [HBr] 1+ A2expBr2 dt Consider the above elementary reactions mechanism proposed by Bodenstein to explain their experimental findings of the reaction rate of HBr. Reactions 1 and 2 are bi-directional (forward and reverse) while reaction 3 is uni-directional (forward only) as written....
A2. Chemical Kinetics (20 marks) MBr2 Br Br M k1 |(1) k2. Br H2 HBr H k2,r (2) k3,f HBr2 HBr Br (3) + Experimentally measured rate expression for [HBr] given as below: d [HBr] A1exp[H2] [Br2]1/2 HBr 1+ A2exp TBr2 dt Consider the above elementary reactions mechanism proposed by Bodenstein to explain their experimental findings of the reaction rate of HBr. Reactions 1 and 2 are bi-directional (forward and reverse) while reaction 3 is uni-directional (forward only) as written....
— O KINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism Suppose the formation of nitrosyl chloride proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + Cl2(9) ► NOCI (9) km 2 NOCI (9) + NO(g) → 2 NOCI (9) kz Suppose also k«k. That is, the first slower than the second 0-0 Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical...
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