---**Kinetics - Determining the Order of Reaction and Rate Constant Calculation**This educational segment aims to elucidate the method of determining the order of a chemical reaction and its corresponding rate constant, \( k \), based on experimental data.### Reaction DataThe data was collected at 580 K for the reaction:\[ 2 \, \text{HI(g)} \rightarrow \text{H}_2(g) + \text{I}_2(g) \]**Table of Data:**| Time (s) | [HI] (mol·L\(^{-1}\)) ||----------|-----------------------|| 0 | 1.00 || 1000 | 0.11 || 2000 | 0.061 || 3000 | 0.041 || 4000 | 0.031 |### Data Analysis1. **Plotting the Data:** Using a graphing calculator or software, plot the concentration of HI against time to determine the reaction order.2. **Determination of Reaction Order:** Plot the data in an appropriate graph: - Zero-order: [HI] vs. Time - First-order: ln[HI] vs. Time - Second-order: \( \frac{1}{[\text{HI}]} \) vs. Time Based on the provided question, it is suggested that the reaction order is 2. Therefore, a second-order reaction graph \( \frac{1}{[\text{HI}]} \) vs. Time should be linear.3. **Graph Interpretation:** Upon plotting, if \( \frac{1}{[\text{HI}]} \) vs. Time yields a straight line, it confirms the reaction is second-order.### Rate Constant CalculationFrom the graph, determine the rate constant, \( k \), for the loss of HI.\[ k = \text{(Slope of the line in the second-order plot)} \]**Example Calculation:**Assuming the line fits the second-order reaction model perfectly, the slope \( k \) can be determined directly from the graph.### Units of Rate ConstantFor a second-order reaction, the units of the rate constant \( k \) are \( \text{L·mol}^{-1}\text{s}^{-1} \).### ConclusionBy plotting the concentration

Solution: Given reaction is 2HI(g) ----> H2(g) + I2(g) Rate=k[A]x where k=rate constant, x=order…

The data in the table were collected at 580 K for the reaction 2 HI(g) → H₂(g) + L₂(g) Time (s) [HI] (mol.L-¹) 0 1.00 1000. 0.11 2000. 0.061 3000. 0.041 4000. 0.031 From the graph, determine the rate constant, k, for the loss of HI. k= TOOLS x10 Using a graphing calculator or software, plot the data in an appropriate fashion to determine the order of the reaction: O 0 O 1 2 Determine the units of the rate constant. mol-L-¹.1 L.mol-¹.s-¹

The data in the table were collected at 580 K for the reaction 2 HI(g) → H₂(g) + L₂(g) Time (s) [HI] (mol.L-¹) 0 1.00 1000. 0.11 2000. 0.061 3000. 0.041 4000. 0.031 From the graph, determine the rate constant, k, for the loss of HI. k= TOOLS x10 Using a graphing calculator or software, plot the data in an appropriate fashion to determine the order of the reaction: O 0 O 1 2 Determine the units of the rate constant. mol-L-¹.1 L.mol-¹.s-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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