Medium
The rate law for a reaction between the substances $A$ and $B$ is given by,$rate = k[A]^n[B]^m$. On doubling the concentration of $A$ and halving the concentration of $B$,the ratio of the new rate to the earlier rate of the reaction will be as
- A$2^{(n - m)}$
- B$2^{(m - n)}$
- C$2^{(n + m)}$
- D$2^{(m + n)}$
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Find the rate law for the reaction,$CHCl_{3(g)} + Cl_{2(g)} \rightarrow CCl_{4(g)} + HCl_{(g)}$ if the order of reaction with respect to $CHCl_{3(g)}$ is $1$ and with respect to $Cl_{2(g)}$ is $1/2$.
For a second-order reaction,the rate constant is $8 \times 10^{-5} \, M^{-1} \, \text{min}^{-1}$. In how much time will a $1 \, M$ solution decrease to $0.5 \, M$?
Medium
View SolutionFor a reaction,$I^{-} + OCl^{-} \to IO^{-} + Cl^{-}$ in an aqueous medium,the rate of reaction is given by $\frac{d[IO^{-}]}{dt} = k[I^{-}][OCl^{-}]$. The overall order of reaction is
Medium
View SolutionThe mechanism of the reaction $A + 2B \to D$ is
$2B \xrightarrow{k} B_2$ $[Slow]$
$B_2 + A \to D$ $[Fast]$
The rate law expression,order with respect to $A$,order with respect to $B$ and overall order of reaction are respectively
$2B \xrightarrow{k} B_2$ $[Slow]$
$B_2 + A \to D$ $[Fast]$
The rate law expression,order with respect to $A$,order with respect to $B$ and overall order of reaction are respectively
Medium
View SolutionIf doubling the concentration of a reactant $A$ increases the rate $4$ times and tripling the concentration of $A$ increases the rate $9$ times,the rate is proportional to
MediumAIIMS 1991
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