For the formation of phosgene from CO g and chlorine- CO g - Cl 2 g - CO Cl 2 g - the experimentally determined rate equation is- d- CO Cl 2 - dt -k- CO - - Cl 2 - 3 - 2-Is the following mechanism consistent with the rate equation- i Cl 2 - 2Cl fast ii Cl-CO- COCl fast iii COCl- Cl 2 - CO Cl 2 -Cl slow

Multiplying equation (ii) by 2 and adding (i) , we get: Cl _ 2 +2CO⇌ 2COCl K=[ COCl ] #160;^ 2 [ Cl _ 2 ] [ CO ] #160;^ 2 ...

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Byju's Answer

Standard X

Chemistry

Metal Oxide and Hydroxide

For the forma...

Question

For the formation of phosgene from $C O (g)$ and chlorine, $C O (g) + {C l}_{2} (g) ⟶ C O {C l}_{2} (g)$ , the experimentally determined rate equation is, $\frac{d [C O {C l}_{2}]}{d t} = k [C O] {[{C l}_{2}]}^{3 / 2}$ .
Is the following mechanism consistent with the rate equation?
$(i)$ ${C l}_{2} ⇌ 2 C l$ (fast)
$(i i)$ $C l + C O ⇌ C O C l$ (fast)
$(i i i)$ $C O C l + {C l}_{2} ⇌ C O {C l}_{2} + C l$ (slow)

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Solution

Multiplying equation $(i i)$ by $2$ and adding $(i)$ , we get:
${C l}_{2} + 2 C O ⇌ 2 C O C l$
$K = \frac{{[C O C l]}^{2}}{[{C l}_{2}] {[C O]}^{2}}$
$[C O C l] = {(K)}^{1 / 2} {[{C l}_{2}]}^{1 / 2} [C O]$ ....(i)
Slowest step is rate determining, hence,
Rate $= k [C O C l] [{C l}_{2}]$ ...(ii)
From equations (i) and (ii), we get
Rate $= k K^{1 / 2} {[{C l}_{2}]}^{1 / 2} [{C l}_{2}] [C O]$
Rate $= k^{^{'}} {[{C l}_{2}]}^{3 / 2} [C O]$
Thus, rate law is in accordance with the mechanism.

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Similar questions

Q. The reaction of formatiom of phosgene from CO and

C l_{2}

C O + C l_{2} \to C O C l_{2}

The proposed mechanism is
(i)

C l_{2} K_{1} - - \to K_{- 1} 2 C l

(fast equilibrium)
(ii)

C l + C O K_{2} - - \to K_{- 2} C O C l

(fast equilibrium)
(iii)

C O C l + C l_{2}_{3} C O C l_{2} + C l

(slow)
The above mechanism leads to the following rate law

\frac{d [C O C l_{2}]}{d t} = K [C O] [C l_{2}]^{3 / 2}

,
Then determine the value of K.

Q. The reaction:

C O + C l_{2} \to C O C l_{2}

has the following mechanism.

What is the rate expression ?

(i)

C l_{2}_{1} K_{2} 2 C l

(fast)
(ii)

C l + C O K_{1}^{'} ⇌ K_{2}^{'} C O C l

(fast)
(iii)

C O C l + C l_{2} K_{3} - \to C O C l_{2} + C l

(slow)

Q. Consider the reaction:

{C l}_{2} (a q .) + H_{2} S (a q .) ⟶ S (s) + 2 H^{+} (a q .) + 2 {C l}^{-} (a q .)

The rate equation for this reaction is:
Rate

= k [{C l}_{2}] [H_{2} S]

Which of these mechanisms is/are consistent with this rate equation?

A

{C l}_{2} + H_{2} S ⟶ H^{+} + {C l}^{-} + {C l}^{+} + H S^{-}

(slow)

{C l}^{+} + H S^{-} ⟶ H^{+} + {C l}^{-} + S

(fast)

B

H_{2} S ⇌ H^{+} + H S^{-}

(fast equilibrium)

{C l}_{2} + H S^{-} ⟶ 2 {C l}^{-} + H^{+} + S

(slow)

Q. The reaction of the formation of phosgene gas from

C O

and

{C l}_{2}

is as follows:

C O (g) + {C l}_{2} (g) ⇌ C O {C l}_{2} (g)

In an experiment, starting with equimolecular

C O

and

{C l}_{2}

in a

250 m L

flask, the equilibrium mixture on analysis is found to contain

0.5 m o l e

C O

0.05

mole

{C l}_{2}

and

0.15

mole

C O {C l}_{2}

. Calculate the equilibrium constant of the reaction.

Q. Consider the reaction :

C l_{2} (a q) + H_{2} S (a q) \to S (s) + 2 H^{+} (a q) + 2 C l^{-} (a q)

The rate equation for this reaction is

= k [C l_{2}] [H_{2} S]

Which of these mechanisms

i s / a r e

consistent with this rate equation?
(A)

C l_{2} + H_{2} S \to H^{+} + C l^{-} + C l^{+} + H S^{-}

(slow)

C l^{+} + H S^{-} \to H^{+} + C l^{-} + S

(fast)
(B)

H_{2} S \Leftrightarrow H^{+} + H S^{-}

(fast equilibrium)

C l_{2} + H S^{-} \to 2 C l^{-} + H^{+} + S

(slow)

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For the formation of phosgene from CO(g) and chlorine, CO(g)+Cl2(g)⟶COCl2(g), the experimentally determined rate equation is, d[COCl2]dt=k[CO][Cl2]3/2.Is the following mechanism consistent with the rate equation?(i) Cl2⇌2Cl (fast)(ii) Cl+CO⇌COCl (fast)(iii) COCl+Cl2⇌COCl2+Cl (slow)