a) Show that the three elementary steps add up to give the overall, stoichiometric equation. b) What is the molecularity of each step? c) For this mechanism to be consistent with kinetic data, what must be the experimental rate equation?

Use the data provided below to determine the most accurate experimental rate law for the reaction: Mix [acetone], (M) [H*], (M) [1,l (M) Rate (M/sec) 1 0.100 0.100 0.00200 0.00374 0.100 0.300 0.00200 0.00374 0.400 0.100 0.00200 0.01496 4 0.100 0.100 0.00600 0.02244 rate = klacetone]°[H*1?tI2] rate = klacetonel[H*][l2] rate = klacetone]l[H*]°[l2]² rate = k[acetone]²[H*]°[l,]² O O O O

A reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. Part A The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. What is the rate law for the following mechanism in terms of the overall rate constant k? Step 1: Step 2: B+ C C ( fast) + D (slow) A +B The exception to this rule occurs when the slowest step contains intermediates. In these cases, the slowest step is usually preceded by an equilibrium step, which can be used to substitute for the intermediates in the overall rate law. Express your answer in terms of k and the necessary concentrations (e.g., k*[A]^3* [D]). • View Available Hint(s) Hνα ΑΣφ ? rate =

Enter an expression for the reaction rate law. Express your answers in terms of k, [NO2], and [F2].

integrated rate law plot for reactant A with time would give you a linear fit? 8) Given the experimental data below, determine the rate law and rate constant (with units) of the reaction. Which Trial [A], M [B], M Initial Rate, M.s1 1 0.10 0.10 0.0019 234 0.20 0.10 0.0081 0.20 0.20 0.0084 0.40 0.30 0.033 Rate Law: Rate Constant: Integrated rate law plot:

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Question:Consider a hypothetical chemical reaction in which compound X reacts with compound Y to form compound Z. The reaction follows a second-order kinetics. If the initial concentration of compound X is doubled while keeping the concentration of compound Y constant, how will this affect the rate of the reaction? Justify your answer using the principles of reaction kinetics

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