Interpretation:
The rate law for the step
Concept Introduction:
The relationship between rate and initial concentration of reactant is described by rate law. It is an experimentally determined equation and cannot be found out theoretically from the stoichiometry of the reactants and products.
Where,
The oxidation reaction of iodide ion by hydrogen peroxide in acidic solution is given below. It is a three step process.
Step
Step
Step
In a multistep reaction, the overall rate of the reaction depends on the rate of the slowest step.
Want to see the full answer?
Check out a sample textbook solutionChapter 11 Solutions
Chemistry: The Molecular Science
- For the reaction of phenyl acetate with water the concentration as a function of time was given in Question 11. Assume that the concentration of water does not change during the reaction. Analyze the data from Question 11 to determine (a) the rate law. (b) the order of the reaction with respect to phenyl acetate. (c) the rate constant. (d) the rate of reaction when the concentration of phenyl acetate is 0.10 mol/L (assuming that the concentration of water is the same as in the experiments in the table in Question 11).arrow_forwardWhen phenacyl bromide and pyridine are both dissolved in methanol, they react to form phenacylpyridinium bromide. When equal concentrations of reactants were mixed in methanol at 35 C, these data were obtained: (a) Determine the rate law for this reaction. (b) Determine the overall order of this reaction. (c) Determine the rate constant for this reaction. (d) Determine the rate constant for this reaction when the concentration of each reactant is 0.030 mol/L.arrow_forwardComplete the following table for the reaction below. It is first-order in both X and Y. 2X(g)+Y(g)productsarrow_forward
- What is the half-life of compound if 75 percent of a given sample of the compound decomposes in 60 min? Assume first-order kinetics.arrow_forwardThe rate law of a reaction is given below.From the given rate law, what will happen to the reaction time and reaction rate if the concentration of one of the reactants is doubled while keeping everything the same? why?Also, why the starch solution used as an indicator in an experiment turned blue at the end of the reaction?arrow_forwardTo get the half-life of a first order reaction, one must divide ln 2 by: a) the initial concentration b) the final concentration c) the rate constant d) the molar mass of the compoundarrow_forward
- A plot of lnk (k is the rate constant) vs 1/T gives a linear graph where the slope is equal to ____________. Activation energy Rate of reaction Entropy of reaction Enthalpy of reactionarrow_forwardWhat is the second order reaction(definition)? Show the equation that represents the rate of following reaction (formation of nitrate radical in the atmosphere)arrow_forwardThe rate constant for first order reaction is 60/s. How much time will it take to reduce the concentration of the reaction to 1/10 of its initial value.arrow_forward
- The half life of a first order reaction is 28 second.what is its rate constant?arrow_forwardEnter your answer in the provided box. Enter your answer in scientific notation. A first-order decomposition reaction has a rate constant of 0.00104 yr−1. What is the half-life of the reaction?arrow_forwardThe following kinetic data were collected at 298 K for the reaction of ozone with nitrite ion, producing nitrate and oxygen: What is the value of the rate Constant? NO2-+O3=NO3-+O2arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher: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
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning