a)The concentration of the starting substance A in a reaction A → products decreasesaccording to Tables a and b, respectively. Determine the reaction order and rateconstants (with units!) for both cases a) and b). Consider both cases separately.t (min)010203040CA (mo/I)0.3120.2210.1560.1100.078b)t (min)CA (mo/I)0103040700.2000.1000.0500.0400.025

OrderRate LawIntegrated Rate LawPlotsSlopeZerothrate = k[A]o - [A]t = kt[A] vs t-kFirstrate =…

Answered: a) The concentration of the starting…

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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[item#2b] *refer to the photo below*
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Chemistry When entering compound units, indicate multiplication of units explicitly using a multiplication dot For example, M^−1⋅s^−1 M^−1⋅s^−1. Express your answer to two significant figures and include the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot or a dash.
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6. The oxidation of Br¯ by Br03 in acidic solution (H*) is described by the equation 5 Br (aq) + Br03 (aq) + 6 H* (aq) З Вrz (aq) + 3 H,0() Initial [Br ] (M) Initial [BrO3] (M) Initial [H*] (M) Initial Reaction Rate (M/s) 4.2 x 10-3 8.4 x 10-3 1.055 x 10-3 4.2 x 10-3 Experiment 1 0.404 0.250 0.100 2 0.808 0.250 0.100 3 0.404 0.125 0.250 0.100 4 0.404 0.050 (a) What is the reaction order with respect to each reactant? (b) Write the rate law. (e) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order
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The following data were obtained at constant temperature for the reaction: 4A(g) + 4B (g) → 3C(g) Initial [A] Initial [B] mol Experiment mol mol Initial Rate L-min L L 1 0.105 0.215 4.50 2 0.315 0.215 13.5 3 0.105 0.430 18.0 4 0.315 0.430 54.0 Part 1 of 2 Select the single best expression for the rate law for the reaction. Ok [A]³ [B]³ G Ok [A] [B] Ok [A] [B] Ok [A][B]²
[item#2a] *refer to the photo below*
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Consider the zero-order reaction, A→ products. The initial concentration of A is 9.98 x 10-3 M and the rate constant = 8.42 x 10-3 M min-1. Calculate the time (min) it takes for the concentration to drop to 3.07 × 10-4 M. Enter the linear form of the integrated rate law for this reaction. Entries in the blanks should include terms only, not units, in the order y, m, x, b. Use brackets as appropriate. = Calculate the time. Report your answer in decimal notation, with proper sig figs. min

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