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.

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Q4.
lodide ions are oxidised to iodine by hydrogen peroxide in acidic conditions.
H₂O₂(aq) + 2H+(aq) + 21-(aq) → 1₂(aq) + 2H₂O(1)
The rate equation for this reaction can be written as
rate = k [H₂O₂] [1] [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.
Transcribed Image Text:Q4. lodide ions are oxidised to iodine by hydrogen peroxide in acidic conditions. H₂O₂(aq) + 2H+(aq) + 21-(aq) → 1₂(aq) + 2H₂O(1) The rate equation for this reaction can be written as rate = k [H₂O₂] [1] [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.
(c)
A graph of the results is shown in Figure 1.
Figure 1
[H+]/mol dm-3
0.5
0.4
0.3-
0.2-
0.1
0.0-
0 50 100 150 200 250 300 350 400 450
time/s
Explain how the graph shows that the order with respect to H*(aq) is zero.
(d) Use the graph in Figure 1 to calculate the value of k₁
Give the units of k₁
K₁
Units
Transcribed Image Text:(c) A graph of the results is shown in Figure 1. Figure 1 [H+]/mol dm-3 0.5 0.4 0.3- 0.2- 0.1 0.0- 0 50 100 150 200 250 300 350 400 450 time/s Explain how the graph shows that the order with respect to H*(aq) is zero. (d) Use the graph in Figure 1 to calculate the value of k₁ Give the units of k₁ K₁ Units
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