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 |
To determine:
Order of reaction of each substance, rate law and rate constant
Explanation of Solution
Let following chemical reaction
Rate law for this reaction can be written as
The rate law for the given reaction can be written as
You have given three set of data. Put each in the above equation
So,
Putting these values on equation, you get
Putting these value in equation you, get
Putting these value in equation you, get
Hence
Hence overall order of reaction
Rate law can be written as
Putting the value
Hence rate law can be written as
It is the initial rates experiment method.
Want to see more full solutions like this?
Chapter 11 Solutions
Bundle: Chemistry for Engineering Students, Loose-Leaf Version, 4th + OWLv2 with MindTap Reader with Student Solutions Manual, 1 term (6 months) Printed Access Card
- Diethylhydrazine reacts with iodine according to the following equation: Â (C2H5)2(NH)2(l)+I2(aq)(C2H5)2N2+2HI(aq)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) What is the order of the reaction with respect to diethylhydrazine, iodine, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. (d) What must [(C2H5)2] be so that the rate of the reaction is 5.00104mol/Lh when [ I2 ]=0.500M?arrow_forwardSubstances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?arrow_forwardThe reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.arrow_forward
- The reaction for the Haber process, the industrial production of ammonia, is N2(g)+3H2(g)2NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 ×10-5 molL-1s-1. At what rate is nitrogen consumed? At what rate is hydrogen consumed?arrow_forwardSome 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 2.01010arrow_forwardAzomethane 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.arrow_forward
- Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.arrow_forwardIn Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research associated with biofuels is the identification and development of suitable catalysts to increase the rate at which fuels can be produced. Do a web search to find an article describing biofuel catalysts. Then, write one or two sentences describing the reactions being catalyzed, and identify the catalyst as homogeneous or heterogeneous.arrow_forward11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.arrow_forward
- The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?arrow_forwardHydrogen bromide is a highly reactive and corrosive gas used mainly as a catalyst for organic reactions. It is produced by reacting hydrogen and bromine gases together. Â H2(g)+Br2(g)2HBr(g)The rate is followed by measuring the intensity of the orange color of the bromine gas. The following data are obtained: (a) What is the order of the reaction with respect to hydrogen, bromine, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. What are the units for k? (d) When [ H2 ]=0.455Mand [ Br2 ]=0.215M, what is the rate of the reaction?arrow_forwardRegular ?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?arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning