Q4. lodide ions are oxidised to iodine by hydrogen peroxide in acidic conditions. H₂O₂(aq) + 2H+(aq) + 21-(aq) → 1₂(aq) + 2H₂O(l) The rate equation for this reaction can be written as rate = k [H₂O₂] [-]³ [H*]c In an experiment to determine the order with respect to H*(aq), a reaction mixture is made containing H*(aq) with a concentration of 0.500 mol dm-3 A large excess of both H₂O₂ and 1- is used in this reaction mixture so that the rate equation can be simplified to rate = k₁ [H*]c (a) Explain why the use of a large excess of H₂O2 and I means that the rate of reaction at a fixed temperature depends only on the concentration of H*(aq). (b) Samples of the reaction mixture are removed at timed intervals and titrated with alkali to determine the concentration of H*(aq). State and explain what must be done to each sample before it is titrated with alkali.
Q4. lodide ions are oxidised to iodine by hydrogen peroxide in acidic conditions. H₂O₂(aq) + 2H+(aq) + 21-(aq) → 1₂(aq) + 2H₂O(l) The rate equation for this reaction can be written as rate = k [H₂O₂] [-]³ [H*]c In an experiment to determine the order with respect to H*(aq), a reaction mixture is made containing H*(aq) with a concentration of 0.500 mol dm-3 A large excess of both H₂O₂ and 1- is used in this reaction mixture so that the rate equation can be simplified to rate = k₁ [H*]c (a) Explain why the use of a large excess of H₂O2 and I means that the rate of reaction at a fixed temperature depends only on the concentration of H*(aq). (b) Samples of the reaction mixture are removed at timed intervals and titrated with alkali to determine the concentration of H*(aq). State and explain what must be done to each sample before it is titrated with alkali.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.96PAE: The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g)...
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