For the reaction: 2A + B to A_2B; the rate = | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The reaction is $2A + B 	o A_2B$. Given the stoichiometry,the change in concentration is $\Delta[A] = [A]_0 - [A]_t = 0.2 - 0.12 = 0.08 \ mol/L$.

Vedclass · Accepted Answer

$3.11 	imes 10^{-8}$

Vedclass · Answer

(A) The reaction is $2A + B 	o A_2B$. Given the stoichiometry,the change in concentration is $\Delta[A] = [A]_0 - [A]_t = 0.2 - 0.12 = 0.08 \ mol/L$. Since $2 \ mol$ of $A$ react with $1 \ mol$ of $B$,the amount of $B$ consumed is $\frac{1}{2} 	imes 0.08 = 0.04 \ mol/L$. Therefore,the concentration of $B$ at this time is $[B]_t = [B]_0 - 0.04 = 0.4 - 0.04 = 0.36 \ mol/L$. The rate law is given by $	ext{Rate} = K[A][B]^2$. Substituting the values: $	ext{Rate} = (2.0 	imes 10^{-6}) 	imes (0.12) 	imes (0.36)^2$. $	ext{Rate} = 2.0 	imes 10^{-6} 	imes 0.12 	imes 0.1296 = 3.1104 	imes 10^{-8} \ mol \ L^{-1} \ s^{-1}$.

$[A_0]$	$0.1 \ M$	$0.025 \ M$
$t_{1/2} \ (s)$	$100 \ s$	$50 \ s$

$Expt. \ No.$	$[A]$	$[B]$	$Initial \ Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

For the reaction: $2A + B \to A_2B$; the rate $= K[A][B]^2$ with $K = 2.0 \times 10^{-6} \ L^2 \ mol^{-2} \ s^{-1}$. Initial concentrations of $A$ and $B$ are $[A]_0 = 0.2 \ mol/L$ and $[B]_0 = 0.4 \ mol/L$ respectively. Calculate the rate of reaction after $[A]$ is reduced to $0.12 \ mol/L$.

Similar Questions

The rate of reaction at $273 \ K$ is $R_0$. The rate of reaction at $313 \ K$ will be (Assuming temperature coefficient equal to $2$).

For a reaction $2 \ A + B \rightarrow P$, when the concentration of $B$ alone is doubled, the rate does not change, and when the concentrations of both $A$ and $B$ are doubled, the rate increases by a factor of $4$. The unit of the rate constant is,

For a certain reaction $A \to P$,the half-life for different initial concentrations of $A$ is mentioned below:
$[A_0]$ $0.1 \ M$ $0.025 \ M$
$t_{1/2} \ (s)$ $100 \ s$ $50 \ s$

Which of the following option$(s)$ is/are correct?

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

For which type of reactions,order and molecularity have the same value?

Vedclass Test Series

Exam Paper Generator

Online Exam Module