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What is the half-life for a particular reaction if the rate law is rate= (1271 M*min) [A] and the initial concentration of A is 0.250 M?

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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Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO, g) +F, (g) NO,F (g) +F (g) k1 2 F (g) + NO, (g) → NO,F (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates.
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Consider the following reaction: 2MnO4–(aq) + 10Br–(aq) + 16H3O+(aq) --> 2Mn2+(aq) + 5Br2(aq) + 24H2O(l) In a reaction under a certain condition, if the rate for the formation of Br2 (D[Br2]/Dt) is 1.0 x 10–5 mol ‧ L–1 ‧ s–1, what is the rate for the disappearance of 2MnO4– (-D[MnO4–]/Dt) in mol ‧ L–1 ‧ s–1 ? (A) 1.0 x 10–5 (B) 4.0 x 10–6 (C) 2.5 x 10–6 (D) 2.5 x 10–5
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