Consider the reaction of peroxydisulfate ion (S2O8-2) with iodide ion (I) in aqueous solution: S2O82- (aq) +
Question:
S2O82- (aq) + 3 Iˉ (aq) -→ 2 SO42- (aq) + I3ˉ(aq)
At a particular temperature the initial rate of disappearance S2O82- of varies with reactant concentrations in the following manner:
(a) Determine the rate law for the reaction and state the units of the rate constant.
(b) What is the average value of the rate constant for the disappearance of S2O82- based on the four sets of data?
(c) How is the rate of disappearance of S2O82- related to the rate of disappearance of Iˉ?
(d) What is the rate of disappearance of Iˉ when [S2O82-] = 0.025 M and [I-] = 0.050 M?
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Step by Step Answer:
a Increasing S 2 O 8 2 by a factor of 15 while holding I constant increases the rat...View the full answer
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Related Book For 
Chemistry The Central Science
ISBN: 978-0321696724
12th edition
Authors: Theodore Brown, Eugene LeMay, Bruce Bursten, Catherine Murphy, Patrick Woodward
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