3Use the following kinetic data to determine the order of the reaction and the value ofthe rate constant.2NOBr (g) 2 NO (g) + Br2 (g)(8Time(s)[NOBr]0102030400.0400.0300.0240.021 0.018[18

Answered: 3 Use the following kinetic data to…

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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At a certain temperature the rate of this reaction is first order in HI with a rate constant of 0.0263 s : 2HI (g) - H, (g)+I, (g) Suppose a vessel contains HI at a concentration of 0.130 M. Calculate the concentration of HI in the vessel 35.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. ) M x10
7 . Please make sure the answer that you give me is correct thank you
25. The reaction 2 NO2(g) + O3(g) N2O5(g) + O2(g) was studied at a certain temperature with the following results: Experiment [NO2(g)] (M) [O3(g)] (M) Rate (M/s) 1 0.502 0.502 21600 2 0.502 1.00 43100 3 1.00 0.502 43100 4 1.00 1.00 85800 (a) What is the rate law for this reaction? Rate = k [NO2(g)] [O3(g)] Rate = k [NO2(g)]2 [O3(g)] Rate = k [NO2(g)] [O3(g)]2 Rate = k [NO2(g)]2 [O3(g)]2 Rate = k [NO2(g)] [O3(g)]3 Rate = k [NO2(g)]4 [O3(g)] (b) What is the value of the rate constant?(c) What is the reaction rate when the concentration of NO2(g) is 0.505 M and that of O3(g) is 1.37 M if the temperature is the same as that used to obtain the data shown above?______ M/s
Use the information provided to calculate the reaction rate. SO2 + 02-S03 Time (s) [SO2] (M) 241 0.532 1050 0.0005 8.63×10-12 10.8×10-6 3.28×10-4 11.9×10-7
Note: This is a The reaction below is first order with respect to NO and second order with respect Cl, Determine the value of the rate constant and write the rate law. 2 NO (2) + Cl2 (g) 2 NOC1 (g) Initial [Cl2] Initial Rate (M/s) Experiment Initial [NO] 0.0125 M- 0.0255 2.27 x 10- 1 0.0125 M 0.0510 9.08 x 10-5 3. 0.0250 M 0.0255 4.55 x 10-5 Rate = 0.00370 M-2s [NO2el [Cl@] Rate = 2.79 M2s [NO2 [Cl(g)] ORate= 0.0712 M-'s [NO] [Clgl* Rate = 5.70 Ms [NOl' [Clze1 Rate = 5.70 M2s [NOl [Cl@l' 2,41 [Cl(e) Rate = 2.79 Ms" [NOe)l' [Cle भजको को तो Rate = 0.00370 M²s [NO2l [Cl2el Rate = 0.0712 M's [NO2] [Cl]
x10 The rate law for the reaction NH(aq) + NO,lag) - N₂ (g) + 2 H₂O (1) is given by rate = k[NH][NO2]. At At a certain temperature, the rate constant is 4.40 × 10-4 1 M.s Calculate the rate of the reaction at that temperature if [NH] = 0.261 M and | [NO]=0 = 0.210 M. Be sure your answer has the correct number of significant digits. G 口・
6)Write the overall rate law for the following reaction: include the units for the rate constant A + B > C Exp [A] [B] rate 1 0.273 0.763 2.83 M/s 0.273 1.526 2.83 M/s 3. 0.819 0.763 25.47 M/s
For A products, time and concentration data were collected and plotted as shown. [A] (M) t (s) 0.900 00.0 0.474 30.0 0.321 60.0 0.243 90.0 t Determine the reaction order, the rate constant, and the units of the rate constant. order= *k = [A] MacBook Pro In[A] t (units) 1/[A] t
A chemistry graduate student is studying the rate of this reaction: 2N,0, (g) 2N,04 (g) +0, (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds: time [N,0,] (milliseconds) 1.00M 10. 0.504M 20. 0.337M 30. 0.253 M 40. 0.203 M
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A chemistry graduate student is studying the rate of this reaction: 2NH₂(g) → N₂(g) + 3H₂(g) She fills a reaction vessel with NH, and measures its concentration as the reaction proceeds: time (milliseconds) 0 10. 20. [NH₂] 0.700M 0.331 M 0.157M 30. 0.0743 M 40. 0.0352M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate=& k= 0 X 님 S

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3 Use the following kinetic data to determine the order of the reaction and the value of the rate constant. 2NOBr (g) 2 NO (g) + Br2 (g) (8 Time(s) [NOBr] 0 10 20 30 40 0.040 0.030 0.024 0.021 0.018 [18