For the reaction A + B rightarrow text{Produc | vedclass

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

Question

(B) The given rate law is $	ext{Rate} = K[A]^1[B]^2$. $1$. If $[B]$ is constant and $[A]$ is doubled,$	ext{Rate}' = K[2A]^1[B]^2 = 2 	imes 	ext{Ra

Vedclass · Accepted Answer

If $[A]$ is kept constant and $[B]$ is reduced to one-fourth,the rate becomes one-fourth of the original rate.

Vedclass · Answer

(B) The given rate law is $	ext{Rate} = K[A]^1[B]^2$. $1$. If $[B]$ is constant and $[A]$ is doubled,$	ext{Rate}' = K[2A]^1[B]^2 = 2 	imes 	ext{Rate}$. This is correct. $2$. If $[A]$ is constant and $[B]$ is reduced to $1/4$,$	ext{Rate}' = K[A]^1[B/4]^2 = K[A]^1[B]^2 / 16 = 	ext{Rate} / 16$. The statement says the rate becomes half,which is incorrect. $3$. If both $[A]$ and $[B]$ are doubled,$	ext{Rate}' = K[2A]^1[2B]^2 = K 	imes 2 	imes 4 	imes [A]^1[B]^2 = 8 	imes 	ext{Rate}$. This is correct. $4$. The overall order of the reaction is $1 + 2 = 3$. This is correct. Thus,the incorrect statement is option $B$.

For the reaction $A + B \rightarrow \text{Product}$,the rate law is given by $\text{Rate} = K[A]^1[B]^2$. Which of the following statements is incorrect?

Similar Questions

For a chemical reaction,the rate law is $\text{rate} = k[A]^2[B]$. If $[A]$ is doubled at constant $[B]$,the rate of reaction:

The reaction $2A + B_{2} \rightarrow 2AB$ is an elementary reaction. For a certain quantity of reactants,if the volume of the reaction vessel is reduced by a factor of $3,$ the rate of the reaction increases by a factor of $.....$. (Round off to the Nearest Integer).

The rate of a gaseous reaction is given by the expression $k[A][B]^{2}$. If the volume of the vessel is reduced to one-half of the initial volume,the reaction rate as compared to the original rate is:

For a reaction between $A$ and $B$,the order with respect to $A$ is $2$ and the order with respect to $B$ is $3$. If the concentrations of both $A$ and $B$ are doubled,the rate will increase by a factor of:

$A$ reaction $2A + B \xrightarrow{k} C + D$ is first order with respect to $A$ and second order with respect to $B$. Initial concentration $(t = 0)$ of $A$ is $C_0$ while $B$ is $2C_0$. If at $t = 30 \min$ the concentration of $C$ is $C_0/4$,then the rate expression at $t = 30 \min$ is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module