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Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![A value of k is found from the rate equation Rate = k[A]M[B]". If m-4 and n-2 and
the unit for the initial rate is M/h. The unit of k is found to be M* h1 (M to the
power of x h to the power of minus 1). What is the value of x?](https://content.bartleby.com/qna-images/question/7a00ba11-4727-4380-bbb0-88ea42161338/9cad42f4-bfa9-48dd-8df5-773c3c50d82d/szptqk_thumbnail.jpeg)
Transcribed Image Text:A value of k is found from the rate equation Rate = k[A]M[B]". If m-4 and n-2 and
the unit for the initial rate is M/h. The unit of k is found to be M* h1 (M to the
power of x h to the power of minus 1). What is the value of x?
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- Consider the reaction 2A + B --> C, where the rate law is RATE = k[A][B]. The unit of the rate constant, k, if the time is measured in minutes is A min 1 M min 1 C M1 min 1 M2 min 1 O A ос « Previous Next B.arrow_forwardBe sure to answer all parts. The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) → 2SO42−(aq) + I3−(aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S2O82−](M) [I−](M) Initial Rate [M/s] 1 0.0200 0.0400 4.80 × 10−4 2 0.0200 0.0200 2.40 × 10−4 3 0.0400 0.0200 4.80 × 10−4 (a) Which of the following equations represents the rate law for this reaction? A. rate = k[S2O82−][I−] C. rate = k[S2O82−][I−]2 B. rate = k[S2O82−]2[I−] D. rate = k[S2O82−]2[I−]2 A B C D (b) What is the rate constant for the reaction? k = /M·sarrow_forwardInitial rate data at 25 ∘C∘C are listed in the table for the reactionNH4+(aq)+NO2−(aq)→N2(g)+2H2O(l)NH4+(aq)+NO2−(aq)→N2(g)+2H2O(l) Experiment Initial [NH4+] Initial [NO2−] Initial Rate of Consumption of NH4+ (M/s) 1 0.24 0.10 7.2×10−67.2×10−6 2 0.12 0.10 3.6×10−63.6×10−6 3 0.12 0.15 5.4×10−6 What is the value of the rate constant?arrow_forward
- Please don't provide handwritten solution .....arrow_forward6arrow_forward[A] [B] Delta [C] / deltat (initial) (M) (M) (m/s) 0.10 0.10 1.04 0.30 0.10 3.1 0.10 0.50 26.0 This is the initial rate data for a rxn: 2 A + 3 B --> 3 C +4 D Now determine the rate law in units of M-2 s-1 [A]2 [B]?arrow_forward
- A+B → Products Run 1 2 3 [A]o [B] (M) (M) 1 1 2 1 2 1 Initial Rate (M/sec) 1 2 4 Rate = k [A]² [B]. What is k (don't forget the units) = [k]?arrow_forwardGiven the following data, estimate the rate constant of A(g) + B(g) → AB(g) (do not write the units in your answer) Experiment [A] (M) [B] (M) Rate (M/s) 1 0.400 0.200 0.8 2 0.200 0.200 0.200 0.200 0.100 0.05arrow_forwardThe integrated rate law is an equation that describes the concentration of a reactant over time (t). The integrated rate law comes in different forms depending on the reaction order. The rate laws below are given for a simple general reaction A-products Order 0 1 2 Integrated rate law [A] = -kt+ [A]o In[A] = − kt+In[A]o =kt+ [A]o Linear graph Slope [A] vs. t -k In[A] vs. t -k V vs. t karrow_forward
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