Difficult
The reaction of hydrogen and iodine monochloride is given as :
$H_{2(g)} + 2ICl_{(g)} \rightarrow 2HCl_{(g)} + I_{2(g)}$
This reaction is of first order with respect to $H_{2(g)}$ and $ICl_{(g)}$. The following mechanisms were proposed:
Mechanism $A$ :
$H_{2(g)} + 2ICl_{(g)} \rightarrow 2HCl_{(g)} + I_{2(g)}$
Mechanism $B$ :
$H_{2(g)} + ICl_{(g)} \rightarrow HCl_{(g)} + HI_{(g)}$ ; (slow)
$HI_{(g)} + ICl_{(g)} \rightarrow HCl_{(g)} + I_{2(g)}$ ; (fast)
Which of the above mechanism$(s)$ can be consistent with the given information about the reaction?
$H_{2(g)} + 2ICl_{(g)} \rightarrow 2HCl_{(g)} + I_{2(g)}$
This reaction is of first order with respect to $H_{2(g)}$ and $ICl_{(g)}$. The following mechanisms were proposed:
Mechanism $A$ :
$H_{2(g)} + 2ICl_{(g)} \rightarrow 2HCl_{(g)} + I_{2(g)}$
Mechanism $B$ :
$H_{2(g)} + ICl_{(g)} \rightarrow HCl_{(g)} + HI_{(g)}$ ; (slow)
$HI_{(g)} + ICl_{(g)} \rightarrow HCl_{(g)} + I_{2(g)}$ ; (fast)
Which of the above mechanism$(s)$ can be consistent with the given information about the reaction?
- A$A$ and $B$ both
- BNeither $A$ nor $B$
- C$A$ only
- D$B$ only
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Similar Questions
The reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:
Experiment $[A] / mol \, L^{-1}$ $[B] / mol \, L^{-1}$ Initial rate / $mol \, L^{-1} \, min^{-1}$ $I$ $0.1$ $0.1$ $2.0 \times 10^{-2}$ $II$ $-$ $0.2$ $4.0 \times 10^{-2}$ $III$ $0.4$ $0.4$ $-$ $IV$ $-$ $0.2$ $2.0 \times 10^{-2}$
| Experiment | $[A] / mol \, L^{-1}$ | $[B] / mol \, L^{-1}$ | Initial rate / $mol \, L^{-1} \, min^{-1}$ |
|---|---|---|---|
| $I$ | $0.1$ | $0.1$ | $2.0 \times 10^{-2}$ |
| $II$ | $-$ | $0.2$ | $4.0 \times 10^{-2}$ |
| $III$ | $0.4$ | $0.4$ | $-$ |
| $IV$ | $-$ | $0.2$ | $2.0 \times 10^{-2}$ |
Difficult
View SolutionThe rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3.0 \times 10^{-4} \ s^{-1}$. If the reaction starts with $1.0 \ mol \ L^{-1}$ of $N_2O_5$,calculate the rate of formation of $NO_2$ at the moment when the concentration of $O_2$ is $0.1 \ mol \ L^{-1}$.
MediumAIIMS 2011
View SolutionWhat will be the overall order of a reaction for which the rate expression is given as $Rate = K[A]^{\frac{1}{2}}[B]^{\frac{3}{2}}$?
The mechanism for the reaction is given below:
$2P + Q \to S + T$
$P + Q \to R + S$ (slow)
$P + R \to T$ (fast)
The rate law expression for the reaction is:
$2P + Q \to S + T$
$P + Q \to R + S$ (slow)
$P + R \to T$ (fast)
The rate law expression for the reaction is:
Medium
View Solution$A_2 + 2 \, B \to 2 \, AB$
$[A_2]$ $[B]$ $-d[A_2]/dt$ $0.1$ $0.2$ $1 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.2$ $2 \times 10^{-2} \, M \, s^{-1}$ $0.2$ $0.4$ $8 \times 10^{-2} \, M \, s^{-1}$
The order of reaction with respect to $A_2$ and $B$ are respectively:
| $[A_2]$ | $[B]$ | $-d[A_2]/dt$ |
|---|---|---|
| $0.1$ | $0.2$ | $1 \times 10^{-2} \, M \, s^{-1}$ |
| $0.2$ | $0.2$ | $2 \times 10^{-2} \, M \, s^{-1}$ |
| $0.2$ | $0.4$ | $8 \times 10^{-2} \, M \, s^{-1}$ |
The order of reaction with respect to $A_2$ and $B$ are respectively:
Medium
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