For the reaction below, the concentration of iodide ion decreases from 1.000 M to 0.868 M...
For the reaction below, the concentration of iodide ion decreases from 1.000 M to 0.868 M in the first 10.0 s.
H2O2 (aq) + 3I-1 (aq)+ 2H+ (aq) --> I3-1 (aq) + 2 H2O (l)
- Calculate the average rate for the disappearance of I-1
- Calculate the average rate of appearance for I3-1
- Calculate the average rate of disappearance of H+
Homework Answers
![H2O₂ (aq) + 3 I (aq) + 2 H+ (aq) Iz laq) + 2 H2011) - 1-0.868 = 0.0132 M/S A3 - 4x0.013) = 4.4 x 10? MIS At TACHT) 2 At ] = 1](http://img.homeworklib.com/questions/72e63900-dce1-11eb-a8a0-1da678a5f5d4.png?x-oss-process=image/resize,w_560)
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For the reaction below, the concentration of iodide ion
decreases from 1.000 M to 0.868 M...
The oxidation of iodide ion by hydrogen peroxide in an acidic solution is described by 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...
Consider this balanced chemical equation: H2O2(?q) + 3I−(?q) + 2H+(?q) → I3−(?q) + 2H2O(?) In the...
Consider this balanced chemical equation: H2O2(?q) + 3I−(?q) + 2H+(?q) → I3−(?q) + 2H2O(?) In the first 10.0 seconds of the reaction, the concentration of I− drops from 1.000 M to 0.868 M. Calculate the average rate of this reaction in this time interval. Determine the rate of change in the concentration of [H+]
Consider the balanced chemical equation. H2O2(aq)+3I−(aq)+2H+(aq)→I3−(aq)+2H2O(l) In the first 14.0 s of the reaction, the concentration...
Consider the balanced chemical equation. H2O2(aq)+3I−(aq)+2H+(aq)→I3−(aq)+2H2O(l) In the first 14.0 s of the reaction, the concentration of I− drops from 1.000 M to 0.817 M Predict the rate of change in the concentration of H2O2 (Δ[H2O2]/Δt). Express the rate to three significant figures and include the appropriate units. (I understand the arithmetic, but I'm having a tough time with the units)
5. 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...
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)...
For the reaction: CH3OH (aq) + H3O+ (aq) + Cl-(aq) --> CH3Cl + 2 H2O (l)...
For the reaction: CH3OH (aq) + H3O+ (aq) + Cl-(aq) --> CH3Cl + 2 H2O (l) The concentration of acid decreases from 2.23 M to 1.89 M in 64.0 s. Calculate the average rate of disappearance of acid Calculate the average rate of appearance of CH3Cl Calculate the average rate of appearance of H2O
The peroxydisulfate ion (S2O82-) reacts with the iodide ion in aqueous solution via the reaction: S2O82-...
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....
7) The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) →...
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−] . ...
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...
[14.38] Consider the reaction of peroxydisulfate ion (S208) with io- dide ion (I) in aqueous solution:...
[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 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...
[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...
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