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Ozonolysis of Aromatics

From the rate...

Question

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
(i) $2 N O (g) \to N_{2} O (g); R a t e = k [N O]^{2}$
(ii) $H_{2} O_{2} (a q) + 3 I^{-} (a q) + 2 H^{+} \to 2 H 2 O (I) + 3 I; R a t e = k [H_{2} O_{2}] [I^{-}]$
(iii) $C H_{3} C H O (g) \to C H_{4} (g) + C O (g); R a t e = k [C H_{3} C H O]^{3 / 2}$
(iv) $C_{2} H_{5} C l (g) \to C_{2} H_{4} (g) + H C l (g); R a t e = k [C_{2} H_{5} C l]$

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Solution

(i) $3 N O (g) \to N_{2} O (g) R a t e = k [N O]^{2}$
Order w.r.t NO is 2 and overall order is 2.
Dimensions of the rate constant
$\frac{m o l L^{- 1}}{s} = k (m o l L^{- 1})^{2} k = m o l^{- 1} L^{1} s^{- 1}$
(ii) $H_{2} O_{2} (a q) + 3 I^{-} (a q) + 2 H^{+} \to 2 H 2 O (I) + I_{3}^{-} R a t e = k [H_{2} O_{2}] [I^{-}]$
Order w.r.t $H_{2} O_{2}$ is 1, order w.r.t $I^{-}$ is 1 and overall order is 2.
Dimensions of the rate constant
$\frac{m o l L^{- 1}}{s} = k (m o l L^{- 1})^{2} k = m o l^{- 1} L^{1} s^{- 1}$
(iii) $C H_{3} C H O (g) \to C H_{4} (g) + C O (g) R a t e = k [C H_{3} C H O]^{3 / 2}$
Order w.r.t $C H_{3} C H O$ is 3/2 and overall order is 3/2.
Dimensions of the rate constant
$\frac{m o l L^{- 1}}{s} = k (m o l L^{- 1})^{3 / 2} k = m o l^{- 1 / 2} L^{1 / 2} s^{- 1}$
(iv) $C_{2} H_{5} C l (g) \to C_{2} H_{4} (g) + H C l (g) R a t e = k [C_{2} H_{5} C l]$
Order w.r.t $C_{2} H_{5} C l$ is 1, and overall order is 1.
Dimensions of the rate constant
$\frac{m o l L^{- 1}}{s} = k (m o l L^{- 1})^{1} k = s^{- 1}$

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Similar questions

Q. Match the rate law given in column I with the dimensions of rate constant given in column II and mark the appropriate choice.

Column I	Column II
(A) $R a t e = k [N H_{3}]^{0}$	(i) $m o l L^{- 1} s^{- 1}$
(B) $R a t e = k [H_{2} O_{2}] [I^{-}]$	(ii) $L m o l^{- 1} s^{- 1}$
(C) $R a t e = k [C H_{3} C H O]^{3 / 2}$	(iii) $s^{- 1}$
(D) $R a t e = k [C_{2} H_{5} C l]$	(iv) $L^{1 / 2} m o l^{- 1 / 2} s^{- 1}$

Q. Identify the reaction order from each of the following rate constants.
(i)

k = 2.3 \times 10^{- 5} L m o l^{- 1} s^{- 1}

k = 3 \times 10^{- 4} s^{- 1}

What is the rate law for a second order reaction: 2A → Products

Q. Find the order of reaction having rate law, rate =

k [N O]^{2} [H_{2}]

Q. Using the data given below the order and rate constant for the reaction

C H_{3} C H O (g) \to C H_{4} (g) + C O (g)

Experiment no.	initial conc (mol/l)	initial rate (mol/l)
1	0.1	0.02
2	0.2	0.08
3	0.3	0.18
4	0.4	0.32

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