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Rate Constant

For the react...

Question

For the reaction $O_{3} (g) + O (g) \to 2 O_{2} (g)$ , if the rate law expression is rate $= k [O_{3}] [O]$ , the molecularity and order of the reaction respectively are:

2 and 2

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2 and 1.33

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2 and 1

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1 and 2

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Solution

The correct option is A 2 and 2
$O_{3} (g) + O (g) \to 2 O_{2} (g)$

Molecularity: The number of reacting species taking part in an elementary reaction, which must collide simultaneously in order to bring about a chemical reaction is called the molecularity of a reaction.
Molecularity is 2 for the above reaction.

Order: The sum of powers of the concentration terms of the reactants in the rate law expression is called the order of that chemical reaction.
The order is 2 for the above reaction.

So, the answer is option, $A$ .

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Similar questions

2 O_{3} (g) \to 3 O_{2} (g)

O_{3} (g) ⇌ O_{2} (g) + O (g)

O_{3} (g) + O s l o w - - \to 2 O_{2} (g)

K [O_{3}]^{2} [O_{2}]^{- 1}

2 O_{3} (g) \to 3 O_{2} (g)

O_{3} (g) ⇌ O_{2} (g) + O (g)

O_{3} (g) + O s l o w - - \to 2 O_{2} (g)

K [O_{3}]^{2} [O_{2}]^{- 1}

2 O_{3} (g) \to 3 O_{2} (g)

O_{3} (g) \to O_{2} (g) + O (g)

O_{3} (g) + O \to^{s l o w} 2 O_{2} (g)

O (g)

K [O_{3}]^{2} [O_{2}]^{- 1}

2 A + 3 B \to

= K (A)^{1} (B)^{2}

A, B

O_{3}

O_{3} (g) + C l (g) ⟶ O_{2} (g) + C l O (g);

k_{1} = 5.2 \times 10^{9} L {m o l}^{- 1} {s e c}^{- 1}

C l O (g) + O (g) ⟶ C l (g) + O_{2} (g);

k_{2} = 2.6 \times 10^{10} L {m o l}^{- 1} {s e c}^{- 1}

O_{3} (g) + O (g) ⟶ 2 O_{2} (g)

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