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In-s [12.5K]
3 years ago
14

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)
Chemistry
1 answer:
LekaFEV [45]3 years ago
8 0

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.

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For the reaction A +B+ C D E, the initial reaction rate was measured for various initial concentrations of reactants. The follow
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Answer:

Rate constant of the reaction is 3.3\times 10^{-3} M^{-2} s^{-1}.

Explanation:

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9.0\times 10^{-5} M/s=k[0.30 M]^a[0.30 M]^b[0.30 M]^c...[1]

Rate(R) of the reaction in trail 2 ,when :

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2.7\times 10^{-4} M/s=k[0.30 M]^a[0.30 M]^b[0.90 M]^c...[2]

Rate(R) of the reaction in trail 3 ,when :

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By [1] ÷ [2], we get value of c ;

c = 1

By [3] ÷ [4], we get value of b ;

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Rate constant of the reaction = k

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k=\frac{9.0\times 10^{-5} M/s}{[0.30 M]^2[0.30 M]^0[0.30 M]^1}

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