The reaction of IC1 with hydrogen 2IC1 + H₂ → I₂ + 2HCI is first order in ICI and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate =

The reaction H3C-1 OHH3C-OH+r may go by either of the following mechanisms: I) H3C-1 H3C++r (slow) H3C++ OH ® H3C-OH (fast) or II) H3C-1+ OHH3C-OH+I* If the first mechanism were correct, what would be the rate law? Rate = K[H3C-1] Rate = K[H3C-1][OH] Rate = k[H3C-1][OH-]2 Rate = K[H3C][OH] Rate = K[H3C+]

Consider the following multistep reaction: C+D = CD (fast) CD +D →CD2 (slow) CD2 + D→CD3 (fast) C+ 3D →CD3 (overall) Based on this mechanism, determine the rate law for the overall reaction. Express your answer in standard MasteringChemistry format. For example, if the rate law is k[C3D]2 type k* [C]^3* [D]^2. • View Available Hint(s)

Be sure to answer all parts. The reaction of peroxydisulfate ion  (S2O82−) with iodide ion (I−) is   S2O82−(aq) + 3I−(aq)  →  2SO42−(aq) + I3−(aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant.  Experiment [S2O82−](M) [I−](M) Initial Rate [M/s] 1 0.0200 0.0400 4.80  ×  10−4 2 0.0200 0.0200 2.40  ×  10−4 3 0.0400 0.0200 4.80  ×  10−4 (a) Which of the following equations represents the rate law for this reaction?  A. rate = k[S2O82−][I−]   C. rate = k[S2O82−][I−]2 B. rate = k[S2O82−]2[I−]   D. rate = k[S2O82−]2[I−]2    A    B    C    D (b) What is the rate constant for the reaction? k =    /M·s

The reaction 2 H2(g) + 2 NO(g) -> 2 H₂O(g) + N2(g) is first order in H₂ and second order in NO. Write the Rate Law for this reaction.

The reaction of nitrogen dioxide with fluorine 2NO2+ F2 → 2NO₂ F is first order in NO2 and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 1.40 × 10-³ M.s¹, when [NO₂] = 2.36 M and [F₂] = 4.12 M. From this experiment, the rate constant is M¹. s-¹

The decomposition of hydrogen peroxide, 2 H₂O(aq) → 2 H₂O(l) + O₂(g), follows first-order kinetics with respect to H2O2 and has k = 0.041 min -1 in the rate law for the decomposition of H₂O2. If the initial concentration of H₂O2 is 0.35 mol/L, what is its concentration after 42 min? Answer in units of mol/L. How much time will it take for the H₂O₂ concentration to decrease from 0.5 mol/L to 0.21 mol/L? Answer in units of min. How much time will it take for the H₂O2 1, concentration to decrease by ? Answer in units of min. How much time will it take for the H₂O2 concentration to decrease by 83%? Answer in units of min.

Order and rate law of a reaction The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is rate = k[NO2]? The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2 is rate = k[NO3]'[C0]! = k[NO3][CO] because the reaction involves only one molecule of each reactant the exponents are omitted. Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 2A→B+ C 2. B +D→E+C

The reaction 2H2(g) + 2NO(g) ----> 2H2O(g) + N2(g) is a first-order in H2 and second order in NO. What is the rate law

The initial concentration of reactant in a first-order reaction is 7.6 M. The rate constant for the reaction is 0.27 s−1. What is the concentration of reactant after 5.51 s? Express your answer in M using at least two significant figures. Do not use scientific notation.