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The Aldol Addition

Consider the ...

Question

Consider the reaction represented by the equation represented by the equation
$C H_{3} C l (g) + H_{2} O (g) \to C H_{3} O H (g) + H C l (g)$
These kinetic data were obtained for the given reaction concentrations
Initial conc (M) Initial conc (M) Initial rate of disappearance of
$[C H_{3} C l]$ $[H_{2} O]$ $C H_{3} C l (M s^{- 1}$
0.2 0.2 1
0.4 0.2 2
0.4 0.4 8
If $H_{2} O$ is taken in large excess, the order of the reaction will be:

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Solution

Comparing the rate law, the order w.r.t. $H_{2} O = 2$ .
w.r.t. $[C H_{3} C l] = 1$
$∴ r = [C H_{3} C l] [H_{2} O]^{2}$
Overall order = 1 + 2 = 3
If $H_{2} O$ is in excess, the order of the reaction will be 1.

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\to

\begin{matrix} S l . N o & [A]_{0} / M (I n i t i a l c o n c .) & [B]_{0} / M (I n i t i a l c o n c .) & R a t e / (M s e c^{- 1}) 1. & 1.6 \times 10^{- 3} & 5 \times 10^{- 2} & 10^{- 3} 2. & 3.2 \times 10^{- 3} & 5 \times 10^{- 2} & 4 \times 10^{- 3} 3. & 1.6 \times 10^{- 3} & 10^{- 1} & 2 \times 10^{- 3} 4. & 3.2 \times 10^{- 3} & 10^{- 1} & 8 \times 10^{- 3} \end{matrix}

2 N O (g) + C l_{2} (g) \to 2 N O C l (g)

Experiment No.	Initial [NO] (M)	Initial $[C_{2}]$ (M)	Initial rate of disappearance of $C l_{2}$ (M/min)
1	0.15	0.15	0.60
2	0.15	0.30	1.20
3	0.30	0.15	2.40
4	0.25	0.25	?

C l_{2}

H_{2} O

C H_{3} C O C H_{3} (a q .) + B r_{2} (a q .) \to

C H_{3} C O C H_{2} B r (a q .) + H^{+} (a q .) + B r^{-} (a q .)

[C H_{3} C O C H_{3}]

[B r_{2}]

[H^{+}]

B r_{2}, M s^{- 1}

5.7 \times 10^{- 5}

5.7 \times 10^{- 5}

1.2 \times 10^{- 4}

3.1 \times 10^{- 4}

A + B ⟶

r = k [A] [B]

B

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Initial conc (M)	Initial conc (M)	Initial rate of disappearance of
$[C H_{3} C l]$	$[H_{2} O]$	$C H_{3} C l (M s^{- 1}$
0.2	0.2	1
0.4	0.2	2
0.4	0.4	8