Consider the following data concerning the equation: H2O2 + 3I– + 2H+ → I3– + 2H2O [H2O2] [I–] [H+] rate I 0.100 M 5.00 × 10–4 M
1.00 × 10–2 M 0.137 M/sec II. 0.100 M 1.00 × 10–3 M 1.00 × 10–2 M 0.268 M/sec III. 0.200 M 1.00 × 10–3 M 1.00 × 10–2 M 0.542 M/sec IV. 0.400 M 1.00 × 10–3 M 2.00 × 10–2 M 1.084 M/sec Two mechanisms are proposed: I. II. Which mechanism and which step as the rate determining step would best fit the data?
1 answer:
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Answer : The correct option is, (C) 6
Explanation :
Oxidation-reduction reaction : It is a reaction in which oxidation and reduction reaction occur simultaneously.
Oxidation reaction : It is the reaction in which a substance looses its electrons. In this oxidation state increases.
Reduction reaction : It is the reaction in which a substance gains electrons. In this oxidation state decreases.
The given unbalanced chemical reaction is,
Half reactions of oxidation and reduction are :
Oxidation : ......(1)
Reduction : .......(2)
In order to balance the electrons, we multiply equation 1 by 2 and equation 2 by 3, we get:
Oxidation : ......(1)
Reduction : .......(2)
The overall balanced chemical reaction will be:
From this reaction we conclude that the electrons are getting transferred from iron to iodine and the number of electrons transferred are 6 electrons.
Hence, the correct option is, (C) 6