## 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...

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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 =
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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
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