Use this graph to answer the following questions:What is the half life of the reaction?Sx10Round your answer to 2 significant digits.Suppose the rate of the reaction is known to be first order inHI. Calculate the value of the rate constant k.k =Round your answer to 2 significant digits. Also be sure youinclude the correct unit symbol.Predict the concentration of HI in the engineer's reactionvessel after 100. seconds have passed.Assume no other reaction is important, and continue to[HI] = []Massume the rate is first order in HI.Round your answer to 2 significant digits. A chemical engineer is studying the rate of this reaction.2HI (g) → H, (g) +I, (g)He fills a reaction vessel with HI and measures its concentration as the reaction proceeds. Here's a graph of his data:0.8-0.6-0.4-0.20.20406080100t (s)Use this graph to answer the following questions:(x) [H]

Use this graph to answer the following questions: What is the half life of the reaction? x10 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 k. k = ? 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 100. seconds have passed. [H1] = ]M Assume no other reaction is important, and continue to assume the rate is first order in HI. Round your answer to 2 significant digits.

Use this graph to answer the following questions: What is the half life of the reaction? x10 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 k. k = ? 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 100. seconds have passed. [H1] = ]M Assume no other reaction is important, and continue to assume the rate is first order in HI. Round your answer to 2 significant digits.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 20QRT

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At 500 K in the presence of a copper surface, ethanol decomposes according to the equation C2H5OH(g)CH3CHO(g)+H2(g) The pressure of C2H5OH was measured as a function of time and the following data were obtained: Time(s) PC2H5OH(torr) 0 250. 100. 237 200. 224 300. 211 400. 198 500. 185 Since the pressure of a gas is directly proportional to the concentration of gas, we can express the rate law for a gaseous reaction in terms of partial pressures. Using the above data, deduce the rate law, the integrated rate law, and the value of the rate constant, all in terms of pressure units in atm and time in seconds. Predict the pressure of C2H5OH after 900. s from the start of the reaction. (Hint: To determine the order of the reaction with respect to C2H5OH, compare how the pressure of C2H5OH decreases with each time listing.)
Chlorine dioxide, ClO2, is a reddish-yellow gas that is soluble in water. In basic solution it gives ClO3 and ClO2 ions. 2ClO2(aq)+2OH(aq)ClO3(aq)+ClO2(aq)+H2O To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Obtain the rate law and the value of 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?
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 reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
Give at least two physical properties that might be used to determine the rate of a reaction.
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
Experimental data are listed here for the reaction A 2 B. (a) Prepare a graph from these data; connect the points with a smooth line; and calculate the rate of change of [B] for each 10-second interval from 0.0 to 40.0 seconds. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. (b) How is the rate of change of [A] related to the rate of change of [B] in each time interval? Calculate the rate of change of [A] for the time interval from 10.0 to 20.0 seconds.
Ammonia is produced by the reaction between nitrogen and hydrogen gases. (a) Write a balanced equation using smallest whole-number coefficients for the reaction. (b) Write an expression for the rate of reaction in terms of [NH3]. (c) The concentration of ammonia increases from 0.257 M to 0.815 M in 15.0 min. Calculate the average rate of reaction over this time interval. (d) Based on your result in part (c), calculate the rate of change of concentration of H2 during the same time interval.
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?
For the reaction of nitrogen monoxide, NO, with chlorine, Cl2, 2NO(g)+Cl2(g)2NOCl(g) the observed rate law is Rate=k[NO]2[Cl2] What is the reaction order with respect to nitrogen monoxide and with respect to Cl2? What is the overall order?