The reaction of IC1 with hydrogen 2IC1 + H₂ → I₂ + 2HCI is first order in ICI and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate =

The reaction of IC1 with hydrogen 2IC1 + H₂ → I₂ + 2HCI is first order in ICI and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. 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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The reaction A + 2B → products was found to be first-order to A and second- order to B. While holding the concentration of A constant, the concentration of B is increased to 5 times its initial value. By what factor does the rate of reaction increase? Please report an integer, without unit.
The reaction of ammonium ion with nitrite ion in aqueous solution NH, +NO, → + N₂+ 2H₂O is first order in NH4 and first order in NO₂. Complete the rate law for this reaction in the box below. Use the form k[A]™ [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 3.72 x 10-5 M-s¹, when [NH₂+] = 0.564 M and [NO₂] = 0.164 M. From this experiment, the rate constant is M¹.s¹ D
The reaction H3C-1 OHH3C-OH+r may go by either of the following mechanisms: I) H3C-1 H3C++r (slow) H3C++ OH ® H3C-OH (fast) or II) H3C-1+ OHH3C-OH+I* If the first mechanism were correct, what would be the rate law? Rate = K[H3C-1] Rate = K[H3C-1][OH] Rate = k[H3C-1][OH-]2 Rate = K[H3C][OH] Rate = K[H3C+]
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Be 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·s
The reaction 2 H2(g) + 2 NO(g) -> 2 H₂O(g) + N2(g) is first order in H₂ and second order in NO. Write the Rate Law for this reaction.
The reaction of nitrogen dioxide with fluorine 2NO2+ F2 → 2NO₂ F is first order in NO2 and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 1.40 × 10-³ M.s¹, when [NO₂] = 2.36 M and [F₂] = 4.12 M. From this experiment, the rate constant is M¹. s-¹
The decomposition of hydrogen peroxide, 2 H₂O(aq) → 2 H₂O(l) + O₂(g), follows first-order kinetics with respect to H2O2 and has k = 0.041 min -1 in the rate law for the decomposition of H₂O2. If the initial concentration of H₂O2 is 0.35 mol/L, what is its concentration after 42 min? Answer in units of mol/L. How much time will it take for the H₂O₂ concentration to decrease from 0.5 mol/L to 0.21 mol/L? Answer in units of min. How much time will it take for the H₂O2 1, concentration to decrease by ? Answer in units of min. How much time will it take for the H₂O2 concentration to decrease by 83%? Answer in units of min.
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