A chemical reaction A-2B - AB2 follows in two steps-A-B - AB slowAB-B - AB2 fastThen the order of the reaction is-

The correct option is B 2Slowest reaction will be rate determining step: A+B → AB [slow] Rate of reaction = k [A] #160; [B] order = 1+1= 2 Orde ...

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Standard XII

Chemistry

Characteristics of Chemical Equilibrium

A chemical re...

Question

A chemical reaction A+2B $\to A B_{2}$ follows in two steps:

A+B $\to$ AB (slow)
AB+B $\to$ $A B_{2}$ (fast)

Then the order of the reaction is:

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Solution

The correct option is B 2
Slowest reaction will be rate-determining step:

$A + B \to A B [s l o w]$

Rate of reaction $= k [A] [B]$

$o r d e r = 1 + 1 = 2$

Order of the reaction can be known from the no. of reactants involved in rate-determining step (slow step).

Hence, option B is correct.

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Similar questions

Q. Study the mechanism of the following reversible reaction carefully

2 A + 2 B ⇌ A_{2} B_{2}

Mechanism

A + B_{f_{1}}

A B + B_{f_{2}}

(slowest step)

A B_{2} + A_{f_{3}}

Rate constant for reaction is:

Q. The two equilibrium

A B ⇋ A^{+} + B^{-}

and

A B + B^{-} ⇋ A B_{2}^{-}

are simultaneously maintained in a solution with equilibrium constant

K_{1}

and

K_{2}

respectively. The ratio of

[A^{+}]

to [

A B_{2}^{-}

] in the solution is:

Q. The two equilibria

A B ⇌ A^{+} + B^{-}

and

A B + B^{-} ⇌ A B_{2}^{-}

are simultaneously maintained in a solution with equilibrium constant

K_{1}

and

K_{2}

respectively. The ratio of

A^{+}

{A B}_{2}^{-}

in the solution is:

Q. The two equilibria

A B ⇌ A^{+} + B^{-}

and

A B + B^{-} ⇌ A B_{2}^{-}

are simultaneously maintained in a solution with equilibrium constants,

K_{1}

and

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respectively. The ratio of

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Q. For a gaseous phase reaction

A + 2 B ⇌ {A B}_{2}

K_{C} = 0.3475 L^{2} {m o l e}^{- 2}

at 200

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. When 2 moles of

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A chemical reaction A+2B→AB2 follows in two steps:A+B → AB (slow)AB+B → AB2 (fast)Then the order of the reaction is:

The correct option is B 2Slowest reaction will be rate-determining step:A+B →AB[slow]Rate of reaction =k[A][B]order=1+1=2Order of the reaction can be known from the no. of reactants involved in rate-determining step (slow step).Hence, option B is correct.

A chemical reaction A+2B $\to A B_{2}$ follows in two steps:

A+B $\to$ AB (slow)
AB+B $\to$ $A B_{2}$ (fast)

Then the order of the reaction is:

The correct option is B 2
Slowest reaction will be rate-determining step:

$A + B \to A B [s l o w]$

Rate of reaction $= k [A] [B]$

$o r d e r = 1 + 1 = 2$

Order of the reaction can be known from the no. of reactants involved in rate-determining step (slow step).

Hence, option B is correct.