The following data was obtained: a. Determine the rate law. B. Calculate the rate constant Experiment...
Consider the reaction of peroxydisulfate ion (S2O8^2-)(Aq) with iodide ion (I-) in aqueous solution: (S2O8^2-)(Aq)+(3I-)(Aq)---->2SO4^2-+(I3-)(Aq).At a particular temperature the rate of disappearance of S2O8^2 varies with reactant concentrations in the following manner:Experiment S2O8^2- I- Initial Rate1 0.018 0.036 2.6x10^-62 0.027 0.036 3.9x10^-63 0.036 0.054 7.8x10^-64 0.050 0.072 1.4x10^-51) Determine the rate law for the reaction.Apparently the rate law is Rate=[S2O8^2-][I-]How did they come up with this?2)How is the rate of disappearance ofS2O8^2- related to the rate of disappearance of [I-]...
[14.38] Consider the reaction of peroxydisulfate ion (S208) with io- dide ion (I) in aqueous solution: S20s (ag) +3I(ag)2 SO4 (ag) +I3 (aq) At a particular temperature the initial rate of disappearance of S2082 varies with reactant concentrations in the following manner Experiment [S208 ] (M UI M Initial Rate (M/s) 2 3 4 0.018 0.027 0.036 0.050 0.036 2.6 x 106 0.036 3.9 x 106 0.054 7.8 x 106 0.072 E4 105 (a) Determine the rate law for the...
Rate Laws (Section)Consider the reaction of peroxydisulfate ion (S2O8 2-) with iodide ion (I - ) in aqueous solution:S2O82 - (aq) + 3 I - (aq)→2 SO42 - (aq) + I3- (aq)At a particular temperature the initial rate of disappearance of S2O8 2 - varies with reactant concentrations in the following manner:Experiment[S2O82‑] (M)[I_] (M)Initial Rate (M/S)10.0180.0362.6 × 10-620.0270.0363.9 × 10-630.0360.0547.8 × 10-640.0500.0721.4 × 10-5(a) Determine the rate law for the reaction and state the units of the rate constant. (b)...
Consider the reaction of peroxydisulfate ion (S20;-) with iodide ion (I) in aqueous solution: S2O3- (aq) + 31- (aq) +250- (aq) +15 (aq). At a particular temperature the rate of disappearance of S20% varies with reactant concentrations in the following manner: 1 Experiment S20%- (M) I- (M) Initial Rate (M/s) 0.018 0.036 2.6 x 10-6 0.027 0.036 3.9 x 10-6 0.036 0.054 7.8 x 10-6 N 3 4 0.050 0.072 1.4 x 10-5 Part D What is the rate of...
Applicati 6. For a generic reaction A + B C, the following data are obtained Experiment Initial /AL. M Initial (e). M Initial rate (M/s 0.100 M 0.100 M 0.100 M 0.200 M 16.0 x 10 16.0 x 10 0200 M 0,100M 64.0 x10 64.0 x 10 0.100 M a. (5 pts) Based on the data, what is the rate law for the reaction? b. (5 pts) using experiment #2's data, solve for k. (5 pts) For experiment #2, after...
The following data were obtained for the reaction A+B → products: Experiment [A]O [B]O Initial rate, v (mol L''s') 2 3 1.25 x 10-3 M 1.25 x 10-3 M 12.50 x 10-3 M 1.25 x 10-3 M 1.25 x 10-3 M 3.13 x 10-3 M 3.01 x 10-3 M1.00 x 10-3 M 0.0087 0.0174 0.0544 4 ? 10.) Write the rate law for the reaction. Explain your reasoning in arriving at your rate law. (Hint: Table 1 is useful here.]...
Using The Following Data, Determine the Rate Law For The Reaction. Part A. 2NO(g)+O(g) --> 2NO2(g) Experiment [NO] [O2] Initial Rate (M/s] 1 0.0126 0.0125 1.41x10^-2 2 0.0252 0.0250 1.13x10^-1 3 0.0252 0.0125 5.64x10^-2 Part B. S2O8charge2-(ag)+3 I charge 1-(aq) ----> 2SO4charge2-(aq)+I3charge1-(aq) Experiment [S2O8charge2-] [ I charge1-] Initial Rate (M/s) 1 0.023 0.048 6.8x10^-6 2 0.054 0.048 1.6x10^-5 3 0.054 0.019 6.3x10^-6
a. Write the rate law for this reaction. b. Calculate the rate constant. c. At what rate does KI disappear if the initial concentrations are [KI] = 0.0450 M and [(NH4)2S2O8] = 0.120 M? d. At what rate does (NH4)2S2O8 disappear under the conditions given in part c? The powers of 10 in the last boxes are 10^-3 Some data for this reaction follows: Experiment INHA.SoJON) T [Kn Initial Rate of Appearance of KL CMU's) 0200 0100 4.76 x 10...
Using the following data, determine the rate law and calculate k: rate = k[F2]x[ClO2]y Experiment [F2] (M) [ClO2] (M) Initial rate (M/s) 1 0.40 0.05 1.2 M/s 2 0.20 0.10 0.60 M/s 3 0.40 0.10 2.4 M/s
From the data table determine the rate law for reactions 1-4 and calculate the value of k for each. Thanks I-IV BACKGROUND INFORMATION Given: 3% H2O2 Concentration= 0.88M & 1.5% H2O2 Concentration= 0.44 M •Calculation of H2O2 after mixing for parts I,II, IV= 0.704 M •Calculation of I^- after mixing for parts I,II, IV= 0.10 M •Calculation of Initial (mol/L-s) Filled in Table Now the solutions for Rate Order and Rate Constant are needed Reactants 8 ml 30% HO, 2...