### Study of Gas Phase Decomposition of Hydrogen Iodide at 700 KIn an investigation of the gas phase decomposition of hydrogen iodide at a temperature of 700 K, the reaction was observed as follows:\[ \text{HI(g)} \rightarrow ½ \text{H}_2\text{(g)} + ½ \text{I}_2\text{(g)} \]**Objective:**To monitor the concentration of hydrogen iodide (HI) as a function of time.**Method:**A graph was created plotting \(\frac{1}{[\text{HI}]}\) against time (in seconds). The results yielded a straight line characterized by:- **Slope:** \(1.64 \times 10^{-3} \, \text{M}^{-1} \text{s}^{-1}\)- **Y-intercept:** \(0.418 \, \text{M}^{-1}\)**Conclusion:**Based on the graph's linearity and slope value, it was determined that:- The reaction is \(\boxed{2}\) order in HI.- The rate constant \(k\) for the reaction is \(\boxed{1.64 \times 10^{-3}} \, \text{M}^{-1} \text{s}^{-1}\).This analysis indicates that as the concentration of HI decreases over time, the rate at which it decomposes can be effectively modeled using a second-order rate law. The slope of the line obtained from the \(\frac{1}{[\text{HI}]}\) vs. time plot provides the rate constant necessary for predicting the kinetics of this reaction under the specified conditions.

Given reaction: HI(g) → 12 H2(g) + 12 I2(g) The slope of the plot of 1/[HI] versus time in seconds…

In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g) →½ H₂(g) + ½ I₂(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.64x10-³ M-¹ s-¹ and a y-intercept of 0.418 M-¹. Based on this plot, the reaction is order in HI and the rate constant for the reaction is M-¹ S-¹.

In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g) →½ H₂(g) + ½ I₂(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.64x10-³ M-¹ s-¹ and a y-intercept of 0.418 M-¹. Based on this plot, the reaction is order in HI and the rate constant for the reaction is M-¹ S-¹.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.58PAE

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