### Chemical Kinetics: Understanding Elementary Reactions#### 52. For a bimolecular elementary reaction, why does the reaction rate depend on the product of the reactant concentrations? Give a very simple example, using numbers, to illustrate your answer.**Explanation:**In a bimolecular elementary reaction, two reactant molecules collide and react to form products. The rate of such reactions depends on how frequently the reactant molecules collide with each other, which in turn depends on their concentrations. Mathematically, the rate $ r $ of a bimolecular reaction involving reactants $ A $ and $ B $ can be expressed as:\[ r = k[A][B] \]Where:- $ k $ is the rate constant.- $[A]$ and $[B]$ are the concentrations of reactants A and B respectively.**Example:**Suppose $ [A] = 2 $ M and $ [B] = 3 $ M, and the rate constant $ k = 1 \, \text{L} \cdot \text{mol}^{-1} \cdot \text{s}^{-1} $.Then, the reaction rate $ r $ can be calculated as:\[ r = (1 \, \text{L} \cdot \text{mol}^{-1} \cdot \text{s}^{-1})(2 \, \text{M})(3 \, \text{M}) = 6 \, \text{M}^2 \cdot \text{L}^{-1} \cdot \text{s}^{-1} \]This illustrates that the reaction rate is proportional to the product of the concentrations of $ A $ and $ B $.#### 53. Why is there no such thing as a trimolecular elementary reaction?**Explanation:**In chemical kinetics, elementary reactions involve a small number of reactant molecules colliding simultaneously. While bimolecular reactions (involving two molecules) are quite common, trimolecular reactions (involving three molecules colliding simultaneously) are extremely rare. The reason is purely probabilistic: the likelihood of three molecules coming together at the exact same moment with the proper orientation and sufficient energy to react is very low. Such events are statistically unlikely in a typical chemical environment.Instead, reactions that appear to involve three or more molecules usually proceed via a series of simpler bimolecular or unimolecular

Answered: Image /qna-images/answer/1896563d-cd8b-4d9c-9e3a-c211b5219dc7.jpg

52. For a bimolecular elementary reaction, why does the reaction rate depend on the product of the reactant concentrations? Give a very simple example, using numbers, to illustrate your answer. 53. Why is there no such thing as a trimolecular elementary reaction?

52. For a bimolecular elementary reaction, why does the reaction rate depend on the product of the reactant concentrations? Give a very simple example, using numbers, to illustrate your answer. 53. Why is there no such thing as a trimolecular elementary reaction?

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...

See similar textbooks

Similar questions

Chapter 15: Chemical Kinetics 54. The tabulated data show the concentration of N₂O5 versus time for this reaction: N₂O5(g) → NO3(g) + NO₂(g) F5 Time (s) 0 25 50 75 100 125 150 175 200 [N₂O5] (M) 1.000 0.822 0.677 0.557 0.458 0.377 0.310 0.255 0.210 Determine the order of the reaction and the value of the rate constant. Predict the concentration of N₂O5 at 250 s. 口 ▶ 4-80^@@@60760@@ - @@G|O@ MacBook Air ➤11
L山 Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2 initial rate of reaction 0.708M 2.02M 71.0M/s 2.29M 2.02M 743.M/s 0.708M 0.571M 20.1M/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. %3D Check Save For Later O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use P. EPIC ... MacBook Pro 888 F4 F3 F5 F10 $ # 3 5. 6. R. ock C B. W. alt option command commar
10. Rate = k [X][Y]0.5 . The reaction order with respect to X is a. 1.5 b. 1.0 С. 0.5 he unkown, contaning at least one of the Group The d. 2.0 e. 0
The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2 and of KI. The data appear below. Determine the rate constant using the data from the first experiment.
Which of the following statements are true about a first-order reaction? X. Units of the rate constant are sec. Y. The time required for reactant to decrease from 0.80 M to 0.60 M is the same as the time required for that reactant to decrease from 0.60 M to 0.40 M. Z. The instantaneous rate is proportional to reactant concentration. X only X and Z only Y and Z only Z only O 0 OO
Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2 initial rate of reaction 0.276M 2.14M 45.0M/s 0.276M 2.54M 63.4 M/s 0.0491M 2.14M 1.42 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|| k = Continue MacBook Air
Decomposition of hydrogen peroxide (H2O2) is a first order reaction. The initial concentration of hydrogen peroxide was 0.350M and after 2 minutes it decomposed to 0.117M. Calculate the fraction consumed. A. 0.755 B. 0.334 C. 0.666 D. 0.253
6. Consider the following mechanism and use it to answer the questions that follow. Step 1: A+A=X Step 2: X+B →→C+Y Step 3: Y+B → D a. Write the overall reaction. b. Identify any species that are reactants, products, intermediates, and/or transition states. c. Write the rate law for this reaction and explain your rationale. [fast] [slow] [fast]
Some measurements of the initial rate of a certain reaction are given in the table below. N₂ [H₂] initial rate of reaction 1.85M 0.232M 1.85M 0.899M 6.27M 0.232M rate=& 3.00M/s 45.0M/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 2 significant digits. Also be sure your answer has the correct unit symbol. k = 0 34.5 M/s G x10 ロ・ロ X 00
Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.88M 1.34M 52.0 M/s 1.88M 0.296M |0.514M| 1.34M rate = k 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 2 significant digits. Also be sure your answer has the correct unit symbol. k = 11.5 M/s 0 3.89 M/s x10 0.0 X
Some measurements of the initial rate of a certain reaction are given in the table below. [N2] H2 initial rate of reaction 0.802M 1.70M 77.0M/s 0.802M 0.476M 21.6M/s 1.77M| 1.70M 375.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 =
What are the units for k in a zero order reaction? * L mol-1 s-1 L3 mol-3 s-1 mol L-1 S-1 None of the above