The 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 are respectively
The 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 are respectively
- A
$K[B]^2, \,0,\, 2,\, 2$
- B
$K[A]' [B]^2,\, 1,\, 2, \,3$
- C
$K[A]^2, \,0, \,2,\, 2$
- D
$K[A]^2[B]^1, \,1, \,2, \,3$
Similar Questions
The reaction, $X + 2Y + Z \to N$ occurs by the following mechanism
$(i)$ $X + Y \rightleftharpoons M$ very rapid equilibrium
$(ii)$ $M + Z \to P$ slow
$(iii)$ $O + Y \to N$ very fast
What is the rate law for this reaction
The reaction, $X + 2Y + Z \to N$ occurs by the following mechanism
$(i)$ $X + Y \rightleftharpoons M$ very rapid equilibrium
$(ii)$ $M + Z \to P$ slow
$(iii)$ $O + Y \to N$ very fast
What is the rate law for this reaction
The results given in the below table were obtained during kinetic studies of the following reaction:
$2 A + B \longrightarrow C + D$
Experiment
$[ A ] / molL ^{-1}$
$[ B ] / molL ^{-1}$
Initial $rate/molL$ $^{-1}$ $\min ^{-1}$
$I$
$0.1$
$0.1$
$6.00 \times 10^{-3}$
$II$
$0.1$
$0.2$
$2.40 \times 10^{-2}$
$III$
$0.2$
$0.1$
$1.20 \times 10^{-2}$
$IV$
$X$
$0.2$
$7.20 \times 10^{-2}$
$V$
$0.3$
$Y$
$2.88 \times 10^{-1}$
$X$ and $Y$ in the given table are respectively :
The results given in the below table were obtained during kinetic studies of the following reaction:
$2 A + B \longrightarrow C + D$
| Experiment | $[ A ] / molL ^{-1}$ | $[ B ] / molL ^{-1}$ | Initial $rate/molL$ $^{-1}$ $\min ^{-1}$ |
| $I$ | $0.1$ | $0.1$ | $6.00 \times 10^{-3}$ |
| $II$ | $0.1$ | $0.2$ | $2.40 \times 10^{-2}$ |
| $III$ | $0.2$ | $0.1$ | $1.20 \times 10^{-2}$ |
| $IV$ | $X$ | $0.2$ | $7.20 \times 10^{-2}$ |
| $V$ | $0.3$ | $Y$ | $2.88 \times 10^{-1}$ |
$X$ and $Y$ in the given table are respectively :
- [JEE MAIN 2020]
The incorrect order indicated against the rate of reaction is Rate Order
$A+B\xrightarrow{K}C$
Rate Order
The incorrect order indicated against the rate of reaction is Rate Order
$A+B\xrightarrow{K}C$
Rate Order
Write differential rate expression of following reaction and give its order of reaction :
$H _{2} O _{2}+ I ^{-} \rightarrow H _{2} O + IO ^{-}$
$H _{2} O _{2}+ IO ^{-} \rightarrow H _{2} O + I ^{-}+ O _{2}$
Write differential rate expression of following reaction and give its order of reaction :
$H _{2} O _{2}+ I ^{-} \rightarrow H _{2} O + IO ^{-}$
$H _{2} O _{2}+ IO ^{-} \rightarrow H _{2} O + I ^{-}+ O _{2}$
$(a)$ Write general reaction and derive the units of rate constant. $(b)$ Based on that write the rate constant for zero, first and $2^{nd}$ order reaction.
$(a)$ Write general reaction and derive the units of rate constant. $(b)$ Based on that write the rate constant for zero, first and $2^{nd}$ order reaction.