The following reaction has a second-order rate law- H2g - 2IClg - I2g - 2HClgRate - k-H2-ICl-Devise a possible reaction mechanism-

Possible reaction mechanism: H_2+ICl⟶ HCl+HI… slow(RDS) HI+ICl⟶ HCl+I_2… fast Hence, Rate=K[H_2][ICl] from rate determining step(rds). ...

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

First Order Reaction

The following...

Question

The following reaction has a second-order rate law:
$H_{2} (g) + 2 I C l (g) \to I_{2} (g) + 2 H C l (g)$
Rate $= k [H_{2}] [I C l]$
Devise a possible reaction mechanism.

Open in App

Solution

Possible reaction mechanism:
$H_{2} + I C l ⟶ H C l + H I \dots s l o w (R D S)$
$H I + I C l ⟶ H C l + I_{2} \dots f a s t$
Hence, $R a t e = K [H_{2}] [I C l]$ from rate determining step(rds).

Suggest Corrections

Similar questions

Q. The reaction at hydrogen and iodine monochloride is represented by the equation is

H_{2} (g) + 2 I C l (g) \to 2 H C l (g) + I_{2} (g)

This reaction is first order in

H_{2} (g)

and also first - order in ICI(g). which of these proposed mechanism can be consistent with the given information about this reaction ?
Mechanism I :

H_{2} (g) + 2 I C l (g) \to 2 H C l (g) + I_{2} (g)

Mechanism II :

H_{2} (g) + I C l (g) s l o w \to H C l (g) + H I (g)

H I (g) + I C l (g) f a s t \to H C l (g) + I_{2} (g)

The reaction of hydrogen and iodine monochloride is given as:
$H_{2} (g) + 2 I C l (g) \to 2 H C l (g) + I_{2} (g)$

This reaction is of first order with respect to $H_{2} (g)$ and $I C l (g)$ , following mechanisms were proposed :
Mechanism A : $H_{2} (g) + 2 I C l (g) \to 2 H C l (g) + I_{2} (g)$

Mechanism B : $H_{2} (g) + I C l (g) \to H C l (g) + H I (g), s l o w$

$H I (g) + I C l (g) \to H C l (g) + I_{2} (g), f a s t$
Which of the above mechanism(s) can be consistent with the given information about the reaction?

The possible mechanism for the reaction:

$2 H_{2 +} 2 N O \to N_{2} + 2 H_{2} O$ is

$(i) 2 N O ⇌ N_{2} O_{2} (i i) N_{2} O_{2} + H_{2} \to N_{2} O + H_{2} O (slow) (i i i) N_{2} O + H_{2} \to N_{2} H_{2} O (fast)$ What is (i) the rate law for the reaction (ii) the order of the reaction?

A following mechanism has been proposed for a reaction

The rate law expression for the reaction is:

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

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

Join BYJU'S Learning Program

The following reaction has a second-order rate law:H2(g)+2ICl(g)→I2(g)+2HCl(g)Rate =k[H2][ICl]Devise a possible reaction mechanism.

Possible reaction mechanism:H2+ICl⟶HCl+HI…slow(RDS)HI+ICl⟶HCl+I2…fastHence, Rate=K[H2][ICl] from rate determining step(rds).

The following reaction has a second-order rate law:
$H_{2} (g) + 2 I C l (g) \to I_{2} (g) + 2 H C l (g)$
Rate $= k [H_{2}] [I C l]$
Devise a possible reaction mechanism.

Possible reaction mechanism:
$H_{2} + I C l ⟶ H C l + H I \dots s l o w (R D S)$
$H I + I C l ⟶ H C l + I_{2} \dots f a s t$
Hence, $R a t e = K [H_{2}] [I C l]$ from rate determining step(rds).