4. You have two reactions that you wish to carry out. Each reaction only involves a single reactant compound. To do this you make two solutions each having an initial concentration of 0.20 M in the reactant. The first reaction is first order and proceeds with a rate constant of 2.0 s-1. The second reaction is second order in the reactant and proceeds with a rate constant of 4.0 M-1s-1. Calculate the initial rate for each reaction. Why does the rate constant with the larger numerical value lead to a slower rate?

4. You have two reactions that you wish to carry out. Each reaction only involves a single reactant compound. To do this you make two solutions each having an initial concentration of 0.20 M in the reactant. The first reaction is first order and proceeds with a rate constant of 2.0 s-1. The second reaction is second order in the reactant and proceeds with a rate constant of 4.0 M-1s-1. Calculate the initial rate for each reaction. Why does the rate constant with the larger numerical value lead to a slower rate?

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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Let’s consider the following reaction, X+2Y - Z After performing some experiments, let’s assume a researcher has determined the rate law for this reaction to be, Rate = k [X][Y]2 But later, a second researcher reports that the mechanism for this reaction is actually, 2Y- 1 (slow) X+1- Z (fast) In the previously determined rate law consistent with this mechanism? If not, why? What should be rate law predicted by this mechanism?
1. Determine the equation for solving the average rate of this reaction 2 N2 Os → 4 NO2+ O2 a. In terms of NO2 formation b. In terms of N2Os decomposition 2. Determine the order for the individual reactants in the following reaction, as well as the overall order of reaction: C2H4 + H2 > C2H6 Note: By experimentation, it was found out that the reaction obeys the following rate law: rate=k [C2H4] [H2]? 3. The reaction 4 OH + H2S → SO2+ 2 H2O + Hz is first order with respect to OH and first order with respect to H2S. a. What is the overall reaction order? b. What is the rate equation for the reaction?
4. Consider three hypothetical reactions of the type A → products. One of the reactions is zeroth order, one is first order, and one is second order. If they all have the same numerical value of the rate constant k (in units of M s ¹, s and M¹s¹, -1 -1 9 respectively), what must be the initial concentration [A]o if the half-lives are equal for a) the zeroth- and first-order reactions, b) the zeroth- and second-order reactions, and c) the first- and second-order reactions.
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Cc.59.
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For the following reaction: 2N2O5(g) ---> 4 NO2(g) + O2(g) The rate law is first order with respect to N2O5 and has a rate constant of 4.82 x 10-3 sec-1 . Calculate the rate of reaction when the [N2O5] = 0.25M.
The decomposition of N2O5 follows the reaction below. 2N2O5 →4NO2 +O2Use the information provided to determine the rate law and rate constant for the decomposition of N2O5.
can you help with 7b