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13 Dec 2019

Consider the reaction of peroxydisulfate ion (S2O2?8) with iodide ion (I?) in aqueous solution:
S2O2?8(aq)+3I?(aq)?2SO2?4(aq)+I?3(aq).
At a particular temperature the rate of disappearance of S2O2?8 varies with reactant concentrations in the following manner:

Experiment S2O2?8(M) I?(M) Initial Rate (M/s)
1 0.018 0.036 2.6×10?6
2 0.027 0.036 3.9×10?6
3 0.036 0.054 7.8×10?6
4 0.050 0.072 1.4×10?5

Part D - What is the rate of disappearance of I? when [S2O2?8]=2.8×10?2 M and [I?]= 5.0×10?2 M ?

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Nestor Rutherford
Nestor RutherfordLv2
17 Dec 2019

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Consider the reaction of peroxydisulfate ion (S2O2−8) with iodide ion (I−) in aqueous solution:
S2O2−8(aq)+3I−(aq)→2SO2−4(aq)+I−3(aq).
At a particular temperature the rate of disappearance of S2O2−8 varies with reactant concentrations in the following manner:

Experiment S2O2−8(M) I−(M) Initial Rate (M/s)
1 0.018 0.036 2.6×10−6
2 0.027 0.036 3.9×10−6
3 0.036 0.054 7.8×10−6
4 0.050 0.072 1.4×10−5

Part A

Determine the rate law for the reaction.

A) rate=k[S2O2−8]2[I−]
B) rate=k[S2O2−8][I−]2
C) rate=k[S2O2−8][I−]
D) rate=k[S2O2−8]2[I−]2

Part B

What is the average value of the rate constant for the disappearance of S2O2−8 based on the four sets of data?

Part C

How is the rate of disappearance of S2O2−8 related to the rate of disappearance of I−?

A) the rate of disappearance of I− is one-third the rate of disappearance of S2O2−8
B) the rate of disappearance of S2O2−8 is one-third the rate of disappearance of I−

C) the rate of disappearance of S2O2−8 is equal to the rate of disappearance of I−

Part D

What is the rate of disappearance of I− when [S2O2−8]= 3.5×10−2 M and [I−]= 5.0×10−2 M ?

Express your answer using two significant figures.

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