Trial [I-] (M) [BrO3-] (M) [H+] (M) 1 1.67*10-3  6.67*10-3  1.67*10-2  2 3.33*10-3  6.67*10-3  1.67*10-2  3 1.67*10-3  1.33*10-2  1.67*10-2  4 1.67*10-3  6.67*10-3  3.33*10-2  Reaction time: Trial 1 - 301.90 secs Trial 2 - 213.28 secs Trial 3 - 214.92 secs Trial 4 - 86.45 secs Calculate the rate for each trial and Using the information above determine the rate law (m, n and p) for the reaction.  m_____________ n_________________ p ____________ Rate= k[I-]m[BrO3-]n[H+]p

Reaction kinetics lab Can anyone help me to answer the question please?

A+B → Products Run 1 2 3 [A]o [B] (M) (M) 1 1 2 1 2 1 Initial Rate (M/sec) 1 2 4 Rate = k [A]² [B]. What is k (don't forget the units) = [k]?

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The following initial rate data are for the reaction of ICI with hydrogen: 2 ICI + Hz I, + 2 HCI Experiment [ICI], M [Ha]o, M Initial Rate, M s-1 1.58×10-2 3.16x10-2 6.29x10-2 0.126 1 0.254 0.188 2 0.508 0.188 3 l0.254 0.375 4 0.508 0.375 Complete the rate law for this reaction in the box below, Use the form k[A]"[B]", where '1' is understood for m orn and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is

Q2: Nitramide decomposes in water according to the chemical equation, kobs N₂O + H₂O 0,N-NH, The observed rate law is the following, The proposed mechanism is: O,N-NH, = 1² +11 d[N₂0] dt = kobs [0,N – NH2] [H+] O,N-NH + H* N₂O O,N-NH H* + OH H₂O Fast Is the reaction mechanism consistent with the observed rate law? If so, what is the relationship between kobs and the rate constants of the individual steps? Fast Equilibrium + он Slow

The reaction S2O82-(aq) + 3 I-(aq)  2 SO42-(aq) + I3-(aq) was studied at a certain temperature with the following results:   Experiment [S2O82-(aq)] (M) [I-(aq)] (M) Rate (M/s)   1 0.0406 0.0406 7.60e-06 2 0.0406 0.0812 1.52e-05 3 0.0812 0.0406 1.52e-05 4 0.0812 0.0812 3.04e-05 (a) What is the rate law for this reaction? Rate = k [S2O82-(aq)] [I-(aq)]Rate = k [S2O82-(aq)]2 [I-(aq)]    Rate = k [S2O82-(aq)] [I-(aq)]2Rate = k [S2O82-(aq)]2 [I-(aq)]2Rate = k [S2O82-(aq)] [I-(aq)]3Rate = k [S2O82-(aq)]4 [I-(aq)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of S2O82-(aq) is 0.0715 M and that of I-(aq) is 0.0834 M if the temperature is the same as that used to obtain the data shown above?  M/s

Please don't provide handwritten solution ....

In general, to calculate the time required for a given initial concentration to decrease by 35% given the rate constant with units of 1/M -1s -1, which equation should be used?   [A] t = -kt + [A] o ln([A] t/[A] o) = – kt Rate = k[A] 1/[A] t = kt + 1/[A] o t 1/2 = ln2/k

Using the data in the table, calculate the rate constant of this reaction. k= A+B C+D Trial 1 2 3 Units [A] (M) 0.260 0.260 0.364 [B] (M) 0.350 0.945 0.350 Rate (M/s) 0.0167 0.122 0.0234