7) 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 | 0.0960 | 7.60 × 10−4 |
2 | 0.0200 | 0.0480 | 3.80 × 10−4 |
3 | 0.0400 | 0.0480 | 7.60 × 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 |
(b) What is the rate constant for the reaction?
a) k = _______ /M · s
7) The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) →...
5. 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 0.0300 0.0840 8.80 × 10−4 2 0.0300 0.0420 4.40 × 10−4 3 0.0600 0.0420 8.80 × 10−4 (a) Which of the following equations represents the rate law for this reaction? What is the...
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...
The peroxydisulfate ion (S2O82-) reacts with the iodide ion in aqueous solution via the reaction: S2O82- (aq) + 3I- → 2SO42- + I3- (aq) An aqueous solution containing 0.050 M of S2O82-ion and 0.072 M of I-is prepared, and the progress of the reaction followed by measuring [I-].The data obtained is given the table below. Time (s) 0.000 400.0 800.0 1200.0 1600.0 [I-] (M) 0.072 0.057 0.046 0.037 0.029 The concentration of S2O82- remaining at 800 s is ________ M....
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)...
q 4 Be sure to answer all parts. The reaction of peroxydisulfate ion (S20s with iodide ion (I) is S20s(aq) + 31(aq) - » 2sO4(aq) + I3 (aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment[S20sj(M IM Initial Rate [M/s] 0.0300 0.0300 0.0600 0.0440 0.0220 0.0220 8.40 × 10-4 4.20 × 10-4 8.40 x 104 (a) Which of the following equations represents the rate law for this reaction? A....
Be sure to answer all parts. The reaction of peroxydisulfate ion (S_2O_8^2-) with iodide ion (I^-)is S_2O_8^2-(aq) + 3I^-(aq) rightarrow 2S0_4^2^-(aq) +I_3^-(aq) From this data collected at a certain temperature, calculate the rate constant.
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...
[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...
The oxidation of iodide ion by hydrogen peroxide in an acidic solution is described by the balanced equation H2O2(aq)+3I−(aq)+2H+(aq)⟶I3−(aq)+2H2O(l)H2O2(aq)+3I−(aq)+2H+(aq)⟶I3−(aq)+2H2O(l) The rate of formation of the red triiodide ion, Δ[I3−]/ΔtΔ[I3−]/Δt, can be determined by measuring the rate of appearance of the color. A sequence of photographs showing the progress of the reaction of hydrogen peroxide (H2O2)(H2O2) and iodide ion (I−)(I−). As time passes (left to right), the red color due to the triiodide ion (I3−)(I3−) increases in intensity. Initial rate data...
In lab you wish to explore kinetic rates of the aqueous reaction between peroxydisulfate(S2O82–) and iodide which produces sulfate and the iodine. You are able to collect the following data: Trial Initial Concentration (M) Initial Rate (M*s^-1) S2O8^2- I- 1 0.15 0.21 1.12 2 0.31 0.21 2.26 3 0.15 0.11 0.57 Using the data provided, what is the rate law for the above chemical reaction? Which species in the reaction (reactants or products) would be most useful in identifying the...