x/Isl.exe/1o_u-IgNslkr7j8P3jH-IQs_dp5pR4ENzvdYC-70kX Bb Logout E Login | Student Veri... PJ Course Home CINBTICS AND EQUILIBRIUM Using a rate law The rate of a certain reaction is given by the following rate law: rate = *[NO] [0,] Use this information to answer the questions below, What is the reaction order in NO? What is the reaction orderin 0,7 What is overall reaction order? At a certain concentrațion of NO and 0,, the initial rate of reaction is 0.120 M/s. What would the initial rate of the reaction be f the concentration of N0 were doubled? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 16.0 M/s when [NO]= 0,045M and [0,] = 1.5 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits,.

x/Isl.exe/1o_u-IgNslkr7j8P3jH-IQs_dp5pR4ENzvdYC-70kX Bb Logout E Login | Student Veri... PJ Course Home CINBTICS AND EQUILIBRIUM Using a rate law The rate of a certain reaction is given by the following rate law: rate = *[NO] [0,] Use this information to answer the questions below, What is the reaction order in NO? What is the reaction orderin 0,7 What is overall reaction order? At a certain concentrațion of NO and 0,, the initial rate of reaction is 0.120 M/s. What would the initial rate of the reaction be f the concentration of N0 were doubled? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 16.0 M/s when [NO]= 0,045M and [0,] = 1.5 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits,.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
At low temperatures, the rate law for the reaction CO(g)+NO2(g)CO2(g)+NO(g)is as follows: rate=(constant)[ NO2 ]2. Which of the following mechanisms is consistent with the rate law? (a) CO+NO2CO2+NO(b) 2NO2N2O4(fast) N2O4+2CO2CO2+2NO(slow) (c) 2NO2NO3+NO(slow) NO3+CONO2+CO2(fast) (d) 2NO22NO+O2(slow) O2+2CO2CO2(fast)
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
Show how equation 20.33 reduces to a simpler form of an integrated first-order rate law when the reverse reaction of an equilibrium is negligible.
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 g ( 0.15106 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant. [Penicillin] (M) Rate (mol/L/min) 2.0106 1.01010 3.0106 1.51010 4.0106 2.01010
Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g)N2(g)+C2H6(g)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time (in hours) that it takes to decrease the concentration to 0.100 M. (d) Calculate the rate of the reaction when [ (CH3)2N2 ]=0.415M.
A proposed mechanism for the gas-phase chlorination of methane is Cl2+CH4CH4Cl+ClCH4ClCH3+HClCH3+Cl2CH3Cl+ClCl+CH4CH3+HCl Suppose the first step is the RDS. What is the expected rate law in terms of the original reactants, Cl2 and CH4? How would you determine if this mechanism might be a potentially correct or, for that matter, a potentially incorrect one?