The reaction of - O - 3- with chlorine atom is given as- O - 3 - g - -Cl- g - - O - 2 - g - -ClO- g - - -160- -160- -160- -160- -160- -160- -160- - k - 1 -5-2- 10 - 9 L mol - -1 sec - -1- ClO- g - -O- g - - Cl- g - - O - 2 - g - - -160- -160- -160- -160- -160- -160- -160- -160- -160- k - 2 -2-6- 10 - 10 L mol - -1 sec - -1-Which of these values is closest to the rate constant of the overall reaction- O - 3 - g - -O- g - - 2 O - 2 - g - 3-1- 10 - 10- 1-4- 10 - 20- 5-2- 10 - 9- 2-6- 10 - 10-

The correct option is C 5.2× 10 ^ 9 k _ 1 [ O _ 3 ][Cl]= d dt [ClO] k _ 2 [ClO][O]= d dt [ClO] k _ 1 [ O _ 3 ][Cl]= k _ 2 [ClO][O] ...

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Order of Reaction

The reaction ...

Question

The reaction of $O_{3}$ with chlorine atom is given as:
$O_{3} (g) + C l (g) ⟶ O_{2} (g) + C l O (g);$ $k_{1} = 5.2 \times 10^{9} L {m o l}^{- 1} {s e c}^{- 1}$
$C l O (g) + O (g) ⟶ C l (g) + O_{2} (g);$ $k_{2} = 2.6 \times 10^{10} L {m o l}^{- 1} {s e c}^{- 1}$
Which of these values is closest to the rate constant of the overall reaction?
$O_{3} (g) + O (g) ⟶ 2 O_{2} (g)$

5.2 \times 10^{9}

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2.6 \times 10^{10}

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3.1 \times 10^{10}

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1.4 \times 10^{20}

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Solution

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Similar questions

2 N O_{2} (g) + O_{3} (g) ⟶ N_{2} O_{5} (g) + O_{2} (g)

N O_{2} (g)

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N O_{2} (g) + O_{3} (g) ⟶ N O_{3} (g) + O_{2} (g)

N O_{3} (g) + N O_{2} (g) ⟶ N_{2} O_{5} (g)

O_{3} (g) ⇌ O_{2} (g) + [O]

N O_{2} (g) + [O] (g) ⟶ N O_{3} (g)

N O_{3} (g) + N O_{2} (g) ⟶ N_{2} O_{5} (g)

Δ H / k J

4 C O (g) + 8 H_{2} (g) ⟶ 3 C H_{4} (g) + C O_{2} (g) + 2 H_{2} O (l)

C (g r a p h i t e) + 1 / 2 O_{2} (g) ⟶ C O (g); Δ H / k J = - 110.5 k J

C O (g) + 1 / 2 O_{2} (g) ⟶ C O_{2} (g); Δ H / k J = - 282.9 k J

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l); Δ H / k J = - 285.8 k J

C (g r a p h i t e) + 2 H_{2} (g) ⟶ C H_{4} (g); Δ H / k J = - 74.8 k J

2 N_{2} O_{5} (g) ⟶ 4 N O_{2} (g) + O_{2} (g)

N O_{2}

5.2 \times 10^{- 3} M

100

2 O_{3} (g) ⟶ 3 O_{2} (g)

O_{3} (g) k ⇌ O_{2} (g) + [O] (g)

O_{3} (g) + [O] k^{'} - -------- \to 2 O_{2} (g)

Δ H / k J

4 C O (g) + 8 H_{2} (g) ⟶ 3 C H_{4} (g) + C O_{2} (g) + 2 H_{2} O (l)

C (g r a p h i t e) + 1 / 2 O_{2} (g) ⟶ C O (g); Δ H / k J = - 110.5 k J

C O (g) + 1 / 2 O_{2} (g) ⟶ C O_{2} (g); Δ H / k J = - 282.9 k J

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l); Δ H / k J = - 285.8 k J

C (g r a p h i t e) + 2 H_{2} (g) ⟶ C H_{4} (g); Δ H / k J = - 74.8 k J

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