A chemical engineer is studying the rate of this reaction. 2HI (g) → H₂(g) + 1₂ (g) He fills a reaction vessel with HI and measures its concentration as the reaction proceeds. Here's a graph of his data: (x) [H] 020- 015- 010- 605- 0- 20 60 : (s) Use this graph to answer the following questions: 10 What is the half life of the reaction? Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in HI, Calculate the value of the rate constant . Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of HI in the engineer's reaction vessel after 120. seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in HI Round your answer to 2 significant digits. 100 5/₂-0³ k= 0 [HI] - M ロ･ロ X 00

A chemical engineer is studying the rate of this reaction. 2HI (g) → H₂(g) + 1₂ (g) He fills a reaction vessel with HI and measures its concentration as the reaction proceeds. Here's a graph of his data: (x) [H] 020- 015- 010- 605- 0- 20 60 : (s) Use this graph to answer the following questions: 10 What is the half life of the reaction? Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in HI, Calculate the value of the rate constant . Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of HI in the engineer's reaction vessel after 120. seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in HI Round your answer to 2 significant digits. 100 5/₂-0³ k= 0 [HI] - M ロ･ロ X 00

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 5P

See similar textbooks

Similar questions

Express the rate of the reaction 2N2O(g)2N2(g)+O2(g) in terms of (b) [ N2O ] (a) [ O2 ]
Hydrogen iodide decomposes when heated, forming H2(g) and I2(g). The rate law for this reaction is [HI]/t = k[HI]2. At 443C, k = 30. L/mol min. If the initial HI(g) concentration is 1.5 102 mol/L, what concentration of HI(g) will remain after 10. minutes?
Rank the following in order of increasing reaction rate. (a) Dynamite exploding (b) Iron rusting (c) Paper burning
Ozone, O3, in the Earths upper atmosphere decomposes according to the equation 2 O3(g) 3 O2(g) The mechanism of the reaction is thought to proceed through an initial fast, reversible step followed by a slow, second step. Step 1: Fast, reversible O3(g) O2(g) + O(g) Step 2: Slow O3(g) + O(g) 2 O2(g) (a) Which of the steps is rate-determining? (b) Write the rate equation for the rate-determining step
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 H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant. Rate [H2OJ [Kll (mL min-’) (mol L ’) (mol L ’) 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066
11.44 A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 4.0 X 10_H s"' at 25°C. What is the half-life for the degradation of DDT in this experiment, in years?
Gaseous NO2 decomposes at 573 K. NO2(g) NO(g) + O2(g) The concentration of NO2 was measured as a function of time. A graph of 1/[NO2] versus time gives a straight line with a slope of 1.1 L/mol s. What is the rate law for this reaction? What is the rate constant?
Isomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph. (a) What is the rate law for this reaction? (b) What is the equation for the straight line in this graph? (c) Calculate the rate constant for this reaction. (d) How long does it take for half of the sample to isomerize? (e) What is the concentration of CH3NC after 1.0 104 s?
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
Consider the decomposition reaction 2X2Y+ZThe following graph shows the change in concentration with respect to time for the reaction. What does each of the curves labeled 1, 2, and 3 represent?
Iodomethane (CH3I) is a commonly used reagent in organic chemistry. When used properly, this reagent allows chemists to introduce methyl groups in many different useful applications. The chemical does pose a risk as a carcinogen, possibly owing to iodomethanes ability to react with portions of the DNA strand (if they were to come in contact). Consider the following hypothetical initial rates data: [DNA]0 ( mol/L) [CH3I]0 ( mol/L) Initial Rate (mol/Ls) 0.100 0.100 3.20 104 0.100 0.200 6.40 104 0.200 0.200 1.28 103 Which of the following could be a possible mechanism to explain the initial rate data? MechanismIDNA+CH3IDNACH3++IMechanismIICH3ICH3++ISlowDNA+CH3+DNACH3+Fast
The decomposition of gaseous dimethyl ether at ordinary pressures is first-order. Its half-life is 25.0 minutes at 500 C: CH3OCH3(g) CH4(g) + CO(g) + H2(g) (a) Starting with 8.00 g of dimethyl ether, what mass remains (in grams) after 125 minutes and after 145 minutes? (b) Calculate the time in minutes required to decrease 7.60 ng (nanograms) to 2.25 ng. (c) What fraction of the original dimethyl ether remains after 150 minutes?