Question

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 $0.22\, Ms^{-1}$, 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. $0.05 \,M^{-2} \,s^{-1}$

Answer 1

Answer: (B)

For reaction; $A+B \longrightarrow $ product

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

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

$\therefore k =\frac{0.22}{0.25}$

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