In this study of the reaction between the iodide ion and persulphate ion: S2O8-2 + 2I-...
In this study of the reaction between the iodide ion and persulphate ion:
S2O8-2 + 2I- → I2 + 2SO4-2
we have chosen to express the rate as the change in the concentration of persulphate ion, S2O8-2, per unit time.
Since persulphate ion is being consumed in the reaction, the concentration is decreasing and the rate of change is negative.
As an equation we can write: Rate = -ΔS2O8-2 / Δt
Give two other ways that the rate of this reaction could be expressed, explain in both words and using an equation as in the example above.
Homework Answers
Solution:
The rates for the given reaction are expressed as,
S2O8^2- + 2I- = I2 + 2 SO4^2-
The rate of reactions can be expressed as,
Rate = + Δ I2 / Δt
Here, since I2 is formed in reaction, hence rate can be expressed in positive terms.
Rate = + 1/2 ΔSO4^2- / Δt
Again, since SO4^2- is formed in reaction, hence can be expressed in positive terms.
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In this study of the reaction between the iodide ion and
persulphate ion:
S2O8-2 + 2I-...
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)...
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...
Consider the following reaction:2 N2O(g) → 2 N2(g)+O2(g)
Consider the following reaction:2 N2O(g) → 2 N2(g)+O2(g)Part AExpress the rate of the reaction in terms of the change in concentration of each of the reactants and products.Express the rate of the reaction in terms of the change in concentration of each of the reactants and products.Rate=12Δ[N2O]Δt=−12Δ[N2]Δt=Δ[O2]ΔtRate=Δ[N2O]Δt=12Δ[N2]Δt=−12Δ[O2]ΔtRate=−Δ[N2O]Δt=−12Δ[N2]Δt=12Δ[O2]ΔtRate=−12Δ[N2O]Δt=12Δ[N2]Δt=Δ[O2]ΔtPart BIn the first 14.0 s of the reaction, 1.9×10−2 mol of O2 is produced in a reaction vessel with a volume of 0.460 L . What is the average rate of the reaction over this time...
Consider the following reaction: 2 N2O(g) → 2 N2(g)+O2(g) A) Express the rate of the reaction...
Consider the following reaction: 2 N2O(g) → 2 N2(g)+O2(g) A) Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. ans: Rate= −1/2 Δ[N2O] / Δt= 1/2 Δ[N2] / Δt = Δ[O2] / Δt B) In the first 13.0 s of the reaction, 1.7×10−2 mol of O2 is produced in a reaction vessel with a volume of 0.440 L . What is the average rate of the reaction over this time interval? ans:...
q 4 Be sure to answer all parts. The reaction of peroxydisulfate ion (S20s with iodide...
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....
In lab you wish to explore kinetic rates of the aqueous reaction between peroxydisulfate(S2O82–) and iodide...
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...
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...
equations that may be useful are: 2I(-)+SO2O8(2-)->I2+2SO4(2-) and I2+2S2O3(2-)->2I(-)+S4O6(2-) THE IODINE CLOCK- REACTION KINETICS IN-LAB GUIDELINES...
equations that may be useful are:
2I(-)+SO2O8(2-)->I2+2SO4(2-)
and
I2+2S2O3(2-)->2I(-)+S4O6(2-)
THE IODINE CLOCK- REACTION KINETICS IN-LAB GUIDELINES (WEEK 1) This is a guide to suggest a format for you to prepare your laboratory notebook so that you can efficiently collect and record the data needed for each part of this experiment. Provide a space for observations. Record all original data directly into the laboratory notebook. Show all post-lab calculations in your laboratory notebook. If you did several trials of the same...
The reaction between hydrogen peroxide and iodide has been investigated by F. Bell, R. Gill, D....
The reaction between hydrogen peroxide and iodide has been investigated by F. Bell, R. Gill, D. Holden, and W. F. K. Wynne-Jones in J. Phys. Chem. 55, 874 (1951): H2O2 + 2I- + 2H+ ----> 2H2O + I2. The reaction proceeds by two parallel mechanisms and leads to the rate law: -d[H2O2]/dt = d[I2]/dt = k1[H2O2][I-] + k2[H2O2][I-][H+]. The rate constants k1 and k2 are observed to vary with ionic strength in the fashion shown in the table. Are these...
Be sure to answer all parts. The reaction of peroxydisulfate ion (S_2O_8^2-) with iodide ion (I^-)is...
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.
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...
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....
equations that may be useful are:
2I(-)+SO2O8(2-)->I2+2SO4(2-)
and
I2+2S2O3(2-)->2I(-)+S4O6(2-)
THE IODINE CLOCK- REACTION KINETICS IN-LAB GUIDELINES (WEEK 1) This is a guide to suggest a format for you to prepare your laboratory notebook so that you can efficiently collect and record the data needed for each part of this experiment. Provide a space for observations. Record all original data directly into the laboratory notebook. Show all post-lab calculations in your laboratory notebook. If you did several trials of the same...
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.
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