Assume that the reactions show below are each an elementary step (though maybe not all for the same overall reaction). What is the molecularity for each reaction? What is the rate law for each reaction? (Note: Radicals are included in rate laws any other chemical would be.) a. H2 + O2 →2 OH- b. OH + H2 → H2O + H• c. Cl2 → 2 Cl- d. H+O2 + M→ HO2 + M

Assume that the reactions show below are each an elementary step (though maybe not all for the same overall reaction). What is the molecularity for each reaction? What is the rate law for each reaction? (Note: Radicals are included in rate laws any other chemical would be.) a. H2 + O2 →2 OH- b. OH + H2 → H2O + H• c. Cl2 → 2 Cl- d. H+O2 + M→ HO2 + 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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For a rate law of the form; rate = k[A]m[B]" the exponents m and n are obtained from a. changes in the rate with changing temperature b. the coefficients and A and B in the balanced equation c. the concentrations of A and B in a single experiment d. changes in the reaction rate for different concentrations of A and B
Please Answer The question below.
20. Consider the following general reaction and data: Exp. 1 2 3 Initial [A] (mol/L) 0.024 0.096 0.024 2A + 2B → C + 3D a. What is the rate law for this reaction? Initial [B] (mol/L) 0.085 0.085 0.170 Initial rate (mol/L.s) 6.0x10-6 9.6x10-5 3.0x10-6 b. Calculate the value of the rate constant with units. (If you did not find the coefficients in (a), assume that the order is 1nd order with respect to each reactant). If the chemical "B" is consumed at a rate of 2.3x10³ mol L-s, calculate the rate of production of the chemical "D".
4. The reaction 2NO (g) + 2H2 (g) - N2 (g) + 2H2O (g) is found experimentally to be second order in NO (g) and first-order in H2 (g). a. Write the rate law for the reaction. b. What is the overall order of the reaction? c. What are the units for the rate constant k? d. If [NO] is doubled (while keeping [H2] constant), by what factor will the reaction rate increase? e. If [H2] is doubled (while keeping [NO] constant), by what factor will the reaction rate increase?
8. Given the following mechanism: step 1 step 2 N202 + H2 - N20 + H20 (slow) step 3 2 NO S N2O2 N20 + H2 - N2 + H20 a. Determine the overall reaction. b. List any intermediates that are in this reaction mechanism? c. Determine the rate law. Note: Intermediates may not appear in rate laws. d. Explain why intermediates may not appear in rate laws.
Some measurements of the initial rate of a certain reaction are given in the table below. H2 12 initial rate of reaction 1.47M 1.17M 36.0M/s 1.47M 4.13M 127. M/s 0.591 M 1.17M 14.5 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k| x10 k = 0
9. A possible mechanism for a reaction is 1. 2 NO N₂O₂ 2. N₂O₂ + H₂ → N₂O + H₂O 3. N₂O + H₂ → N₂ + H₂O (fast reaction) (slow reaction) (fast reaction) a. What is the molecularity of the slow step? b. What is the overall reaction? c. Are there any intermediates? If yes, identify the intermediate(s). d. Are there any catalysts? If yes, identify the catalyst (s). e. What is the rate law for the overall reaction based on this mechanism?
For the reaction 2 X --- Y + Z, the rate constant is 0.0543 L.mol-1s-1 at 23 oC. The rate constant increases to 0.1086 L.mol-1s-1 at 33 oC. What is the frequency factor for the reaction? A. 1.78 x 108 B. 9.30 x 107 C. 7.85 x 108 D. 8.80 x 107 E. 6.84 x 109
6. The rate law for the overall reaction 2 N2O5 (g) →4 NO2 (g) + O2 (g) is Rate = k[N2O5). a. Consider this mechanism: i. N2O5 (g) → NO: (g) + NO2 (g) ii. NO2 (g) + N2Os (g) →3 NO2 (g) + O2 (g) i. NO: (g) +0 (g) → NO2 (g) + O2 (g) Is this reaction mechanism consistent with the rate law? Why or Why not? [fast) [slow] [fast] b. If the reacuion mechanism is not consistent with the rate law, how would it need to change to become consistent? c. List potential reaction intermediates present in uNIS nechanism d. Draw a reaction energy diagram for this mechanism including any modifications you've made in a-c.
Based on the following mechanism write out the rate law for the overall reaction. Also identify any catalysts or intermediates. Step 1. A + B -› C Slow Step 2. B + C -› D Fast Step 3. 2D -› E Very Fast
Q3. Consider the reaction: 2C(s) +3H2(g) → C2H6(g) At a certain point, the H2 is being consumed a rate of -0.35moles/minute. What is the rate of C being consumed? Of ethane being produced?
8. Smelling salt decomposes spontaneously at room temperature by the equation below. A student places a 10.00-g sample into a 1-liter sealed rigid vessel. What measurements should the student make to determine the rate of this reaction?(NH4)2CO3(s)→2NH3(g)+H2O(g)+CO2(g) a. change in mass and temperature b. temperature and time c. change in mass and time d. change in pressure and time