Medium
The reaction $A_2 + B_2 \rightarrow 2AB$ follows the mechanism $A_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2A$ (fast),$A + B_2 \xrightarrow{k_2} AB + B$ (slow),$A + B \rightarrow AB$ (fast). The overall order of the reaction is:
- A$1.5$
- B$3$
- C$2.5$
- D$2$
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Similar Questions
The reaction $2 \ NO + Br_2 \rightarrow 2 \ NOBr$ takes place through the mechanism given below:
$NO + Br_2 \Leftrightarrow NOBr_2$ (fast)
$NOBr_2 + NO \rightarrow 2 \ NOBr$ (slow)
The overall order of the reaction is $.....$.
$NO + Br_2 \Leftrightarrow NOBr_2$ (fast)
$NOBr_2 + NO \rightarrow 2 \ NOBr$ (slow)
The overall order of the reaction is $.....$.
In a reaction,the concentration of reactant is increased two times and three times,then the increases in the rate of reaction were four times and nine times respectively. The order of reaction is:
Medium
View SolutionConsider the reaction $2 \ A + 2 \ B \rightarrow C + 2 \ D$. If the concentration of $A$ is doubled at constant $B$,the rate increases by a factor of $4$. If the concentration of $B$ is doubled at constant $A$,the rate is doubled. What is the rate law?
The rate law equation for a reaction between $A$,$B$ and $C$ is $r = k[A][B][C]^2$. What will be the new rate of reaction if the concentration of both $A$ and $B$ are doubled (in $r$)?
Match List-$I$ with List-$II$:
List-$I$ (Order of Reaction) List-$II$ (Unit of rate constant) $A$. Zero order $I$. $mol^{-1} L s^{-1}$ $B$. First order $II$. $mol^{-2} L^{2} s^{-1}$ $C$. Second order $III$. $s^{-1}$ $D$. Third order $IV$. $mol L^{-1} s^{-1}$
| List-$I$ (Order of Reaction) | List-$II$ (Unit of rate constant) |
| $A$. Zero order | $I$. $mol^{-1} L s^{-1}$ |
| $B$. First order | $II$. $mol^{-2} L^{2} s^{-1}$ |
| $C$. Second order | $III$. $s^{-1}$ |
| $D$. Third order | $IV$. $mol L^{-1} s^{-1}$ |
MediumNEET 2026
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