## Understanding Reaction Rates### IntroductionIn the study of chemical kinetics, understanding the rate of reactions is crucial. The rate of a reaction can be determined by examining the change in concentration of reactants over time. Here, we will explore how the initial rate of a reaction depends on the concentration of reactant \( A \).### Reaction DataConsider the following data showing the initial rate of the reaction \( A \rightarrow \text{products} \) for varying concentrations of \( A \).| \([A] \, (\text{M})\) | Initial rate \((\text{M/s})\) ||-----------------|---------------------|| 0.100 | \( 2.02 \times 10^{-2} \) || 0.200 | \( 4.04 \times 10^{-2} \) || 0.300 | \( 6.06 \times 10^{-2} \) |### Determining Reaction OrderThe initial rates suggest a linear relationship between the concentration of \( A \) and the rate, indicating a first-order reaction. Mathematically, this can be expressed as:\[ \text{rate} = k[A]^1 \]where \( k \) is the rate constant.### Part C: Calculating the Rate Constant \( k \)To calculate the value of the rate constant \( k \) for a first-order reaction, use the initial rate data and the relationship:\[ k = \frac{\text{rate}}{[A]} \]Ensure that your answer is expressed in inverse seconds (s\(^{-1}\)) and rounded to three significant figures.### ConclusionUnderstanding the relationship between reactant concentration and reaction rate is essential for determining the order of a reaction and its rate constant, both of which are foundational concepts in chemical kinetics.

Answer:Rate constant is the specific rate of the reaction when reactant concentration of the all the…

MISSED THIS? Watch KCV: The Rate Law for a Chemical Reaction, IWE: Determining the Order and Rate Constant of a Reaction ; Read Section 15.3. You can click on the Review link to access the section in your e Text. Consider the data showing the initial rate of a reaction ( A → products) at several different concentrations of A. [A] (M)Initial rate (M/s) 0.100 2.02 × 10-2 0.200 4.04 x 10-2 0.300 6.06 × 10-2 ▼ Submit k[A] k[A] ✓ Correct As was determined in Part A, the reaction is a first-order reaction, so n = 1 Part C Previous Answers k = rate = k[A]¹ where k is the rate constant. Estimate the value of the rate constant k. Express your answer in inverse seconds to three significant figures. 195) ΑΣΦ ? 8-1

MISSED THIS? Watch KCV: The Rate Law for a Chemical Reaction, IWE: Determining the Order and Rate Constant of a Reaction ; Read Section 15.3. You can click on the Review link to access the section in your e Text. Consider the data showing the initial rate of a reaction ( A → products) at several different concentrations of A. [A] (M)Initial rate (M/s) 0.100 2.02 × 10-2 0.200 4.04 x 10-2 0.300 6.06 × 10-2 ▼ Submit k[A] k[A] ✓ Correct As was determined in Part A, the reaction is a first-order reaction, so n = 1 Part C Previous Answers k = rate = k[A]¹ where k is the rate constant. Estimate the value of the rate constant k. Express your answer in inverse seconds to three significant figures. 195) ΑΣΦ ? 8-1

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

The data in the table below were obtained for the reaction: A + B → PRODUCT Experiment Number [A] (M) |[B] (M)| (M/s) |Initial Rate 1 0.273 0.763 2.83 0.273 1.526 2.83 0.819 0.763 25.47 The rate law for this reaction is rate =
Please help to understand
8 OKONETICS AND EQUILIBRIUM Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2N₂O, (g) → 2N₂O, (g) + O₂(g) He fills a reaction vessel with N₂O, and measures its concentration as the reaction proceeds: time (minutes) 0 10. [N₂O,] Explanation 0.300M 0.121 M 20. 0.0762 M 30. 0.0555 M 40. 0.0436M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. Check rate & D www-awa.aleks.com k= D.D X
1.Study the reaction and read the statement. 2A + 3B + C →→ D + E The rate constant for this reaction is 0.25. The reaction is second order in A and first order in B and C. What is the rate of the reaction if [A] is 0.4 M, [B] is 0.1 M and [C] is 0.2 M? 5.0 × 10–4 4.0 × 10–3 2.0 × 10–3 8.0 × 10, –4
Consider the reaction 2 A + B → C. What is the rate law given the following experimental data? [A], M 0.180 [B], M 0.250 0.180 0.500 0.720 0.500 A. rate = [A]²[B]² ✓B. rate = [A]¹[B]¹ C. rate = [A]²[B]¹ D. rate = [A]¹[B]² rate, M/s 1.36 x 10 2.72 x 10-3 1.09 x 10-2
22. Be sure to answer all parts.The reaction2A + 3B → C is first order with respect to A and B. When the initial concentrations are [A] = 1.70 × 10−2 M and [B] = 2.27 × 10−3 M, the rate is 4.33 × 10−4 M/s. Calculate the rate constant of the reaction.Enter your answer in scientific notation.
8. Given the initial rate data for the reaction A + B → C, determine the rate law for the reaction. [A] Initial Rate 1.31 x 104 5.24 × 104 1.31 x 104 [B] 0.0460 0.220 0.0920 0.220 0.0460 0.440
2NOCl(g) → 2NO(g) + Cl2(g) Rate = k[NOCl]2If this gaseous system has an initial rate of decomposition of NOCl of 0.0010 M s-1, and the volume of the system is reduced to one fifth of its original value, what is the new initial rate of decomposition of NOCl? Assume the temperature remains the same. 5.0×10-3 M s-1 2.5×10-2 M s-1 2.0×10-4 M s-1 4.0×10-5 M s-1 1.0×10-1 M s-1
Some measurements of the initial rate of a certain reaction are given in the table below. [N-] H2 initial rate of reaction 4 0.756M 0.169M 5.00 x 10*M/s 0.186M 0.169M 3.03 × 10°M/s olo 0.756M 0.0761 M 2.25 x 10*M/s Ar 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 [] Ox10 k = 0
Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [N] [H] initial rate of reaction 0.977 M 1.26 M 0.162 M/s 2.87 M 1.26 M 1.40 M/s 0.977 M 2.13 M 0.274 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 = kO k = 0 Explanation Check O 2021 McGraw-Hill Education, All Rights Type here to search 立

Answer all questions in this section. 1. (a) H2S(aq) + Cl2(g) – S(s) + 2HCI(aq) i. Given that, when the concentration of H2S is doubled, rate also double while double the concentration Cl2 will cause the rate of reaction increase 4 times. Write the rate law of the reaction. ii. The overall reaction order ii. The rate of reaction at 300K if the rate constant is 2.8 x 10²M²s' and the concentration of H2S and Cl2 are 2.7×10²M and 7.0x10² M respectively.
2 3 4 =5 #1 6 7 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0040 M-s¹: 2 HI (g) → H₂(g) + 1₂ (g) Suppose a 5.0 L flask is charged under these conditions with 300. mmol of hydrogen iodide. How much is left 4.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. S A S ? Continue Submit 00 X