![(13). if we look to the Rxn: S2O8 (aq)3 1 (aq) 2SO4 (aq) + I3 (aq) 2- We can write the rate of reaction as: Rate=k [S2Os2]1](http://img.homeworklib.com/questions/0a114820-4984-11eb-b9e9-59864ec68eab.png?x-oss-process=image/resize,w_560)
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(13). if we look to the Rxn: S2O8 (aq)3 1 (aq) 2SO4 (aq) + I3 (aq)...
Find the values m , n and the over all order of reaction? (13). if we...
Find the values m , n and the over all order of reaction?
(13). if we look to the Rxn: 2- 2- S2Os(aq)3 I (aq) 2SO4 (aq) I3 (aq) 2-m Rate k [S2Os1" [I 1" We can write the rate of reaction as: Experimental Data for this Reaction are: Initial Conc.,M Initial rate Expt. S20s2 S2Os0.038 [S2Os212=0.076 S2O0.060 -1 Ms [I] [I] 0.060 [I 12=0.060 Ri 1.4 x10 1 R2-2.8 x10 2 R3 4.4x10 [I ]3=0.120 3 Find the values...
S2O8^-2(aq)+3I^-(aq)--2SO4^-2(aq)+I3^-(aq) S2O8^-2. I^- rate 0.018M. &
S2O8^-2(aq)+3I^-(aq)--2SO4^-2(aq)+I3^-(aq) S2O8^-2. I^- rate 0.018M. 0.018M. 2.6*10^-6 0.018M. 0.036M. 5.3*10^-6 0.072M. 0.036M. 2.12*10^-5 a. write the rate law for this reaction including the reaction order for each reactant b. calculate the value of k c. calculate the Rate of the concentration when [S2O8^-2]= 0.2500M and [I]= 0.120M
37. The data below were determined for the reaction shown below. The rate law for this...
37. The data below were determined for the reaction shown below. The rate law for this reaction 12 Marks must be: s2or" + 31-(aq)-25042-+13- Initial Rate 1.4 × 10-5 M/s 2.8 × 10-5 MS 1.4 x 10-5M/s 0.060 0.060 0.030 0.038 0.076 0.076 2 a. Rate kIS 0s I] b. Rate kIS20s IUT *d. Rate = k[S2082-11
I have a reaction that has three elementary steps: 3I- +S2O82- ---> I3- + 2 SO42-...
I have a reaction that has three elementary steps: 3I- +S2O82- ---> I3- + 2 SO42- (this is the RLS) I3 + 2 S2O32- ---> 3 I- + S4O62- starch + I3- ---> starch - I3- complex. (color change to indicate rxn is over) In multiple trials I change the concentrations to see its effect on the rate of the rxn. But the reagents I'm using in this rxn are: (1) starch, Na2S2O3 , KI, KNO3 , and (2) (NH4)2S2O8...
The oxidation of bromide ion by persulfate is given by the equation: S2O82–(aq) + 3Br–(aq) ...
The oxidation of bromide ion by persulfate is given by the
equation: S2O82–(aq) + 3Br–(aq) 2SO4–(aq) + Br3–(aq)
What is the rate law for this reaction based on the following
experimental data?
1. The oxidation of bromide ion by persulfate is given by the equation: S2082-(aq) + 3Br (aq) + 2504 (aq) + Br3 (aq) What is the rate law for this reaction based on the following experimental data? Expt # (S2082-) (Br"] Initial rate mol/L mol/L mol/(L-sec) 1...
The following reaction was studied experimentally at 25 °C. S2O82(aq) + 21'(ag) = 12(aq) + 2SO4...
The following reaction was studied experimentally at 25 °C. S2O82(aq) + 21'(ag) = 12(aq) + 2SO4 (aq) The reaction was found to be first order with respect to I and first order with respect to S208". A reaction was performed with [1] = 0.080 M and [S208²-] = 0.040 M. The initial rate of formation of 12 was found to be 1.25 x 10-M St. Provide an expression for the rate law for this reaction and determine the initial rate...
Rate of Disappearance/Rate Constant
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-]...
Rate Laws (Section)Consider the reaction of peroxydisulfate ion (S2O8 2-) with iodide ion (I - )...
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)...
Preliminary: Key Chemical Equations Reaction 2 Fe3 (a)3 I(a)2 Fe(aq) + I3'(aq) I3(ag) 2 S2032(aq) 3 1a)S4O(0) R...
Preliminary: Key Chemical Equations Reaction 2 Fe3 (a)3 I(a)2 Fe(aq) + I3'(aq) I3(ag) 2 S2032(aq) 3 1a)S4O(0) Reaction 2: + + Prelab Questions 1. List and define any new terms relevant to this experiment 2. Write the general formula for the rate law for Reaction 1 (given above) 3. Write the general formula for calculating average rate bases on the disappearance of thiosulfate (S2O,2) in Reaction 2 (given above) 4. Write the equation used for calculating a concentration after dilution...
The reaction of peroxydisulfate ion (S2O82-) with iodide ion (I -) is given below. S2O82-(aq) +...
The reaction of peroxydisulfate ion
(S2O82-) with iodide ion (I
-) is given below.
S2O82-(aq) + 3 I
-
2SO24-(aq)
+I3-
The following data are collected at a certain temperature.
Experiment
[S2O82- ](M)
[I- ](M)
Initial Rate (M/s)
1
0.080
0.034
2.2 X 10-4
2
0.080
0.017
1.1 X 10-4
3
0.16
0.017
2.2 X 10-4
Determine the rate law.
____________________
Calculate the rate constant.
______________ /(M·s)
The reaction of peroxydisulfate ion (S2O8^2-) with iodide ion (I -) is given...
Find the values m , n and the over all order of reaction?
(13). if we look to the Rxn: 2- 2- S2Os(aq)3 I (aq) 2SO4 (aq) I3 (aq) 2-m Rate k [S2Os1" [I 1" We can write the rate of reaction as: Experimental Data for this Reaction are: Initial Conc.,M Initial rate Expt. S20s2 S2Os0.038 [S2Os212=0.076 S2O0.060 -1 Ms [I] [I] 0.060 [I 12=0.060 Ri 1.4 x10 1 R2-2.8 x10 2 R3 4.4x10 [I ]3=0.120 3 Find the values...
37. The data below were determined for the reaction shown below. The rate law for this reaction 12 Marks must be: s2or" + 31-(aq)-25042-+13- Initial Rate 1.4 × 10-5 M/s 2.8 × 10-5 MS 1.4 x 10-5M/s 0.060 0.060 0.030 0.038 0.076 0.076 2 a. Rate kIS 0s I] b. Rate kIS20s IUT *d. Rate = k[S2082-11
The oxidation of bromide ion by persulfate is given by the
equation: S2O82–(aq) + 3Br–(aq) 2SO4–(aq) + Br3–(aq)
What is the rate law for this reaction based on the following
experimental data?
1. The oxidation of bromide ion by persulfate is given by the equation: S2082-(aq) + 3Br (aq) + 2504 (aq) + Br3 (aq) What is the rate law for this reaction based on the following experimental data? Expt # (S2082-) (Br"] Initial rate mol/L mol/L mol/(L-sec) 1...
The following reaction was studied experimentally at 25 °C. S2O82(aq) + 21'(ag) = 12(aq) + 2SO4 (aq) The reaction was found to be first order with respect to I and first order with respect to S208". A reaction was performed with [1] = 0.080 M and [S208²-] = 0.040 M. The initial rate of formation of 12 was found to be 1.25 x 10-M St. Provide an expression for the rate law for this reaction and determine the initial rate...
Preliminary: Key Chemical Equations Reaction 2 Fe3 (a)3 I(a)2 Fe(aq) + I3'(aq) I3(ag) 2 S2032(aq) 3 1a)S4O(0) Reaction 2: + + Prelab Questions 1. List and define any new terms relevant to this experiment 2. Write the general formula for the rate law for Reaction 1 (given above) 3. Write the general formula for calculating average rate bases on the disappearance of thiosulfate (S2O,2) in Reaction 2 (given above) 4. Write the equation used for calculating a concentration after dilution...
The reaction of peroxydisulfate ion
(S2O82-) with iodide ion (I
-) is given below.
S2O82-(aq) + 3 I
-
2SO24-(aq)
+I3-
The following data are collected at a certain temperature.
Experiment
[S2O82- ](M)
[I- ](M)
Initial Rate (M/s)
1
0.080
0.034
2.2 X 10-4
2
0.080
0.017
1.1 X 10-4
3
0.16
0.017
2.2 X 10-4
Determine the rate law.
____________________
Calculate the rate constant.
______________ /(M·s)
The reaction of peroxydisulfate ion (S2O8^2-) with iodide ion (I -) is given...
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