Question

The overall reaction of ozone reacting to form oxygen has been proposed to occur in a reaction mechanism of: What is the role of O(g) and what is the overall balanced equation? Question 14 options: 1) O(g) is an intermediate; 2O3(g) + O(g)→3O2(g) + O(g) 2) O(g) is a catalyst; 2O3(g) + O(g)→3O2(g) + O(g) 3) O(g) is an intermediate; 2O3(g)→3O2(g) 4) O(g) is a catalyst; 2O3(g)→3O2(g)

Answer 1

Answer:

3) O(g) is an intermediate; 2O3(g)→3O2(g)

Explanation:

The decomposition of ozone to yield oxygen occurs in a sequence of steps. The various non-elementary reactions involved constitute the reaction mechanism. In the sequence of reaction steps O(g) serves as an intermediate.

The overall reaction involves the conversion of two moles of ozone to three moles of oxygen as shown in the answer. Thus the O(g) is merely a reaction intermediate.

Answer 2

The role of O (g) is as an intermediate in the reaction

The overall balanced equation of the reaction is:

2 O₃(g) ----> 3 O₂ (g)

The overall reaction of ozone reacting to form oxygen has been proposed to occur in a reaction mechanism involving two steps:

Step 1: O₃ (g) → O₂ (g) + O (g)

Step 2: 0₃ (g) + O (g) → 2 0₂ (g)

The overall balanced equation of the reaction is:

2 O₃(g) ----> 3 O₂ (g)

A reaction intermediate is an entity formed in a reaction from the reactants of that reaction and which subsequently reacts to form products.

O (g) is produced in step 1 of the reaction of the formation of oxygen from ozone, and is subsequently used in the next step to form products.

Therefore, the role of O (g) is as an intermediate in the reaction.

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