Rate law for the reaction, $A + B ⟶$ product is rate $= k {[A]}^{2} [B]$ . What is the rate constant; if rate of reaction at a given temperature is $0.22 M s^{- 1}$ , when $[A] = 1 M$ and $[B] = 0.25 M$ ?

3.52 M^{- 2} s^{- 1}

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0.88 M^{- 2} s^{- 1}

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1.136 M^{- 2} s^{- 1}

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0.05 M^{- 2} s^{- 1}

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Solution

The correct option is B $0.88 M^{- 2} s^{- 1}$
For reaction; $A + B ⟶$ product
$\frac{d x}{d t} = k {[A]}^{2} [B] \Rightarrow 0.22 = k {(1)}^{2} (0.25)$
$∴ k = \frac{0.22}{0.25} = 0.88 M^{- 2} s^{- 1}$

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Q. Rate law for the reaction

A + B \to P r o d u c t

is,

r a t e = k [A]^{2} [B]

. What is the rate constant, if rate of the reaction at a given temperature is

0.22 M s^{- 1}

, when

[A] = 1 M

and

[B] = 0.25 M

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