For the theoretical reaction: 2BD+F a plausible 2-step reaction mechanism was determined to be 1. A+B=C+D 2. B+C → A+F (slow) Based on this mechanism, what is the predicted rate law for the reverse of the first elementary step? Rate = K[B][C] Rate = K[B]²[D]¹ Rate = K[A][B]²[D] ¹ Rate = K[B]² Rate = K[A][B] Rate = K[C][D] The rate law cannot be determined.

For the theoretical reaction: 2BD+F a plausible 2-step reaction mechanism was determined to be 1. A+B=C+D 2. B+C → A+F (slow) Based on this mechanism, what is the predicted rate law for the reverse of the first elementary step? Rate = K[B][C] Rate = K[B]²[D]¹ Rate = K[A][B]²[D] ¹ Rate = K[B]² Rate = K[A][B] Rate = K[C][D] The rate law cannot be determined.

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...

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Consider the following chemical equation: Overall Reaction: A B2 + BC - AB + C + B2 The proposed mechanism is as follows: BC – B+ C (slow) A B2 + B = AB+ B2 (fast) What is the rate law? Rate = k[B C] O Rate = k[A B,][B] Rate = k[C] O Rate = k[B][C] Rate k[A B2][B C) Rate = k[A B][B,] Rate = k(A B2]
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It was found that for the reaction 2 A + B → 3 C the rate law is Rate = k[A][B] · %3D At the initial concentrations [A]o = 0.100 M and [B]o = 0.200 M the initial rate is 0.0500 M/s. %3D What would be the initial rate if the initial concentrations were [A]o = 0.500 M and [B]o = 0.0750 M? 0.0352 M/s 0.0937 M/s O 0.0711 M/s 0.00533 M/s O 0.469 M/s
The reaction A + 2B → products has been found to have the rate law, rate = k[A] [B]2. While holding the concentration of A constant, the concentration of B is increased from x to 3x. By what factor does the rate of reaction increase? 3 fold 6 fold 9 fold 27 fold the rate of reaction does not change with a change in the [B].
Give answer to all parts
Given the following proposed mechanism, predict the rate law for the overall reaction. Rate = k [A] [C] Rate = k [A] [B]² [C] [E] Rate = k [B] [C] Rate = k [B] [E], Rate = k [A]¹/2 [C] A2B fast B+CD+ E slow B+E F fast
The exponents in a rate law describe the effects of the reactant concentrations on the reaction rate and define the reaction order. Consider a reaction for which the rate law is: rate = k[A]m[B]n If m is 1, the reaction is first order with respect to A. If the exponent is 2, the reaction is second order with respect to A. If n is 1, the reaction is first order in B. If m or n is zero, the reaction is zero order in A or B. If m = 1 and n = 1, the overall order of the reaction is second. (m + n = 1 + 1 = 2). 1. What is the difference between a reaction rate and a reaction's rate constant? 2. What does it mean if a reaction is zero order with respect to a reactant? 3. Doubling the concentration of a reactant increases the rate of a reaction four times. What is the order of the reaction with respect to that reactant? 4. Doubling the concentration of a reactant increases the rate of a reaction four times. Tripling the concentration of a different reactant increases the rate of a reaction…
A valid mechanism for the following overall reaction is given below. Overall reaction: 2 NO (g) + Cl2 (g) → 2 NOCI (g) Step 1: NO (g) + Cl2 (g) → NOCI2 (g) Step 2: NOC12 (g) + NO (g) → 2 NOCI (g) (slow) (fast) What is the rate law for this reaction? Rate = k[NO]?[Cl2] Rate = k[NO][CI] Rate = k[NO][Cl2][NOCI] Rate = k[Cl2][NOC12]