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 Ms-1, when [A]=1 M and [B] = 0.25 M

Question

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 Ms-1, when [A]=1 M and [B] = 0.25 M (A) 3.52 M-2 s-1 (B) 0.88 M-2 s-1 (C) 1.136 M-2 s-1 (D) 0.05 M-2 s-1

Tardigrade Admin · Accepted Answer

For reaction; A+B longrightarrow product (d x/d t) =k[A]2[B] ⇒ 0.22= k(1)2(0.25) ∴ k =(0.22/0.25) =0.88 M -2 s -1

Q. Rate law for the reaction $A + B$ $\to$ 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 $[B] = 0.25 M$

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

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

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

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

For reaction; $A + B ⟶$ product

$\frac{d x}{d t} = k [A]^{2} [B]$

$\Rightarrow 0.22 = k (1)^{2} (0.25)$

$∴ k = \frac{0.22}{0.25}$

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

Q. 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 0.22Ms−1, when [A]=1 M and [B]=0.25M

3.52M−2s−1

0.88M−2s−1

1.136M−2s−1

0.05M−2s−1