18. The rate expression for the reaction,3A2 + 2B2 → 2A, B2, is Rate = k [A2] [B2]2Which one of the following reactions is the rate de-temining step in the mechanism of this reaction?A) A,B + 1/2 B2 A,B2BY A2 + 1/2 B2→ A,BC) A2 + B2 → A,B2D) Az + B2 → 2ABE) A2 + 2B2 2AB2%3D

B option would be correct i.e, A2+1/2B2 --> A2B

3A2 +2B2 2A, B2, is Rate = k (Al [B22 Which one of the following reactions is the rate de termining step in the mechanism of this reaction? A) A2B + 1/2 B, A,B2 BY A2 + 1/2 B2 C) A2 + B2 A,B2 D) A2 + B2 + 2AB E) A2 + 2B2 2AB2 A,B

3A2 +2B2 2A, B2, is Rate = k (Al [B22 Which one of the following reactions is the rate de termining step in the mechanism of this reaction? A) A2B + 1/2 B, A,B2 BY A2 + 1/2 B2 C) A2 + B2 A,B2 D) A2 + B2 + 2AB E) A2 + 2B2 2AB2 A,B

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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2 A(aq) + 3 B(aq) A2B3(aq) An experiment is conducted at 25 C and the rate of appearance of the product ABa(aq) is measured as the concentrations of the reactants were varied. Data from the trials are shown below. Initial Rate of Trial [A] (M) [B] (M) Appearance of A2B3 (M/s) 5.0 x 10 4.5 x 10 1.0 x 10 0.200 0.300 0.200 0.900 0.400 0.300 4 0.135 0.225 ??? Determine the rate law for the reaction. Justify your answer. Determine the value of k, including units. Determine the rate of Trial 4. a. b. с. d. Determine the initial rate of disappearance of A for trial 2. A possible reaction mechanism has a 1" elementary step as shown below: e. A +BAB Could this first step be the rate determining step? Explain your reasoning. In the reaction mechanism the compound MnO2 appears. A student makes the claim f. "The order of MnO2 must be zero since it does not appear in the overall balanced equation". Do you agree or disagree with the student? Explain your reasoning. g. In trial 1, 10 mL of A and 10…
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Which equation is used to determine the amount of time required for the initial concentration to decrease by 45% if the rate constant has units of s⁻¹? A) t = ln 2/k B) Rate = k[A] C) ln([A]/[A]₀) = -kt D) [A] = [A]₀ - kt E) 1/[A] = 1/[A]₀ + kt
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The reaction, A + 2 B → products, has the rate law, rate = k(A)2(B)1. When the concentration of A is tripled, while that of B doubled, by what factor will the rate of the reaction increase? (A) 5 (B) 24 (C) 12 (D) 18 (E) 6