Medium
The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -
Step-$1$ : $A + E \rightleftharpoons AE$ (fast)
Step-$2$ : $AE + A \to A_2 + E$ (slow)
Step-$3$ : $A_2 + B \to C + D$ (fast)
What rate law best agrees with this mechanism?
Step-$1$ : $A + E \rightleftharpoons AE$ (fast)
Step-$2$ : $AE + A \to A_2 + E$ (slow)
Step-$3$ : $A_2 + B \to C + D$ (fast)
What rate law best agrees with this mechanism?
- A$r = k[A][B]$
- B$r = k[A][E]$
- C$r = k[A]^2[E]$
- D$r = k[A]^2[B]$
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Similar Questions
Which one of the following is wrongly matched?
Medium
View SolutionDuring the kinetic study of the reaction,$2A + B \rightarrow C + D,$ the following results were obtained:
$Run$ $[A] / mol \ L^{-1}$ $[B] / mol \ L^{-1}$ Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$ $I.$ $0.1$ $0.1$ $6.0 \times 10^{-3}$ $II.$ $0.3$ $0.2$ $7.2 \times 10^{-2}$ $III.$ $0.3$ $0.4$ $2.88 \times 10^{-1}$ $IV.$ $0.4$ $0.1$ $2.40 \times 10^{-2}$
Based on the above data,which one of the following is correct?
| $Run$ | $[A] / mol \ L^{-1}$ | $[B] / mol \ L^{-1}$ | Initial rate of formation of $D / mol \ L^{-1} \ min^{-1}$ |
| $I.$ | $0.1$ | $0.1$ | $6.0 \times 10^{-3}$ |
| $II.$ | $0.3$ | $0.2$ | $7.2 \times 10^{-2}$ |
| $III.$ | $0.3$ | $0.4$ | $2.88 \times 10^{-1}$ |
| $IV.$ | $0.4$ | $0.1$ | $2.40 \times 10^{-2}$ |
Based on the above data,which one of the following is correct?
For the reaction $A + B \xrightarrow{K} C$,identify the incorrect order of reaction indicated against the rate expression.
Easy
View Solution$A_{(g)} + 2B_{(g)} \to$ product is an elementary reaction. Which of the following is incorrect?
Medium
View SolutionThe following data was obtained for the chemical reaction given below at $975 \ K$: $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_{2}O_{(g)}$
Experiment $[NO] \ (mol \ L^{-1})$ $[H_{2}] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ s^{-1})$ $1$ $8 \times 10^{-5}$ $8 \times 10^{-5}$ $7 \times 10^{-9}$ $2$ $24 \times 10^{-5}$ $8 \times 10^{-5}$ $2.1 \times 10^{-8}$ $3$ $24 \times 10^{-5}$ $32 \times 10^{-5}$ $8.4 \times 10^{-8}$
The order of the reaction with respect to $NO$ is ..... .
| Experiment | $[NO] \ (mol \ L^{-1})$ | $[H_{2}] \ (mol \ L^{-1})$ | Rate $(mol \ L^{-1} \ s^{-1})$ |
| $1$ | $8 \times 10^{-5}$ | $8 \times 10^{-5}$ | $7 \times 10^{-9}$ |
| $2$ | $24 \times 10^{-5}$ | $8 \times 10^{-5}$ | $2.1 \times 10^{-8}$ |
| $3$ | $24 \times 10^{-5}$ | $32 \times 10^{-5}$ | $8.4 \times 10^{-8}$ |
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