Question

For the reaction, $2A+B\to$ products, when the concentrations of A and B both where doubled , the rate of the reaction increased from $0.3mol{L}^{-1}{s}^{-1}$ to $2.4mol{L}^{-1}{s}^{-1}$. When the concentration of A alone is doubled, the rate increased from $0.3mol{L}^{-1}{s}^{-1}$ to $0.6mol{L}^{-1}{s}^{-1}$
Which one of the following statements is correct ?

• A. Order of the reaction with respect to $B$ is $2$
• B. Order of the reaction with respect to $A$ is $2$
• C. Total order of the reaction is $4$
• D. Order of the reaction with respect to $B$ is $1$

Answer 1

Answer: (A)

$r=K[A{]}^x[B{]}^y$
$\Rightarrow 8=2^3=2^{x+y}$
$\Rightarrow x+y=3$ ...(1)
$\Rightarrow 2=2^x$
$\Rightarrow x=1,y=2$
Order w.r.t. $A=1$
Order w.r.t. $B=2$