Medium
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)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?
- ARate $= k[Z]$
- BRate $= k[X][Y]^2[Z]$
- CRate $= [N]$
- DRate $= k[X][Y][Z]$
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Similar Questions
Which of the following rate laws has an overall order of $0.5$ for a reaction involving substances $x$,$y$,and $z$?
MediumAIIMS 1983
View SolutionConsider the following reaction: $A \longrightarrow \text{Products}$. This reaction is completed in $100 \ min$. The rate constant of this reaction at $t_1 = 10 \ min$ is $10^{-2} \ min^{-1}$. What is the rate constant (in $min^{-1}$) at $t_2 = 20 \ min$?
In a reaction between $A$ and $B$,the initial rate of reaction $(r_0)$ was measured for different initial concentrations of $A$ and $B$ as given below:
$A / mol \ L^{-1}$ $0.20$ $0.20$ $0.40$ $B / mol \ L^{-1}$ $0.30$ $0.10$ $0.05$ $r_0 / mol \ L^{-1} \ s^{-1}$ $5.07 \times 10^{-5}$ $5.07 \times 10^{-5}$ $1.43 \times 10^{-4}$
What is the order of the reaction with respect to $A$ and $B$?
| $A / mol \ L^{-1}$ | $0.20$ | $0.20$ | $0.40$ |
| $B / mol \ L^{-1}$ | $0.30$ | $0.10$ | $0.05$ |
| $r_0 / mol \ L^{-1} \ s^{-1}$ | $5.07 \times 10^{-5}$ | $5.07 \times 10^{-5}$ | $1.43 \times 10^{-4}$ |
What is the order of the reaction with respect to $A$ and $B$?
Difficult
View SolutionFor a hypothetical reaction,$A \rightarrow C$. The mechanism is: $A \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} B$ (Fast),$A + B \xrightarrow{k_3} C$ (Slow). The rate law for this reaction is:
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
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