The oxidation of \(\mathrm{SO}_{2}\) to \(\mathrm{SO}_{3}\) is accelerated by \(\mathrm{NO}_{2} .\) The reaction proceeds according to: $$ \begin{array}{l}{\mathrm{NO}_{2}(g)+\mathrm{SO}_{2}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{SO}_{3}(g)} \\ {2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)}\end{array}$$ (a) Show that, with appropriate coefficients, the two reactions can be summed to give the overall oxidation of \(S O_{2}\) by \(\mathrm{O}_{2}\) to give \(S O_{3} .(\mathbf{b})\) Do we consider \(N O_{2}\) a catalyst or an intermediate in this reaction? (c) Would you classify NO as a catalyst or as an intermediate? { ( d ) } Is this an example of homogeneous catalysis or heterogeneous catalysis?

Step by step solution

01

(a) Finding the overall reaction

First, let's balance the two given reactions: 1. NO₂(g) + SO₂(g) → NO(g) + SO₃(g) (already balanced) 2. 2NO(g) + O₂(g) → 2NO₂(g) (already balanced) Now we can sum the reactions. In order to cancel the NO(g) and NO₂(g) species, we need two of the first reaction to balance the second reaction: 2(NO₂(g) + SO₂(g) → NO(g) + SO₃(g)) 2NO(g) + O₂(g) → 2NO₂(g) Summing the reactions, we get: 2NO₂(g) + 2SO₂(g) + 2NO(g) + O₂(g) → 2NO(g) + 2SO₃(g) + 2NO₂(g) Now we can cancel the species present on both sides: 2SO₂(g) + O₂(g) → 2SO₃(g) This is the overall reaction for the oxidation of SO₂ to SO₃.

02

(b) Identifying NO₂ as a catalyst or an intermediate

A catalyst is a substance that increases the rate of a chemical reaction but remains unchanged at the end of the reaction. Looking at the overall reaction, we can see that NO₂ does not appear in the final reaction. Since it is utilized in the first reaction and regenerated in the second, it is a catalyst in this reaction.

03

(c) Identifying NO as a catalyst or an intermediate

An intermediate is a reaction species that is produced during a reaction and is then consumed in a subsequent reaction. NO is produced in the first reaction and consumed in the second reaction, so it is an intermediate in this set of reactions.

04

(d) Classifying the type of catalysis

Homogeneous catalysis occurs when the catalyst and the reactants are in the same phase (e.g., both are gases, liquids, or solids), while heterogeneous catalysis occurs when the catalyst and the reactants are in different phases. In this case, all species are gases, so this is an example of homogeneous catalysis.

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