Medium
The rate of the simple reaction,$2NO + O_2 \to 2NO_2$,when the volume of the reaction vessel is doubled:
- Awill grow eight times of its initial rate
- Breduce to one-eighth of its initial rate
- Cwill grow four times of its initial rate
- Dreduce to one-fourth of its initial rate
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For the reaction $A + B \xrightarrow{K} C$,identify the incorrect order of reaction indicated against the rate expression.
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View SolutionWhy is molecularity applicable only for elementary reactions,while order is applicable for both elementary and complex reactions?
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View SolutionFor the reaction $AB_5 \to AB + 4B$,if $- \frac{d[AB_5]}{dt} = K_1[AB_5]$ and $\frac{d[B]}{dt} = K_2[AB_5]$,then:
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View SolutionIf $r = k[A]^2[B]$ is the rate law equation for the reaction $A + B \rightarrow C$,at $[A] = 1 \ M$ and $[B] = 0.2 \ M$,calculate the rate of reaction if the rate constant is $6.25 \ M^{-2} \ s^{-1}$. (in $M \ s^{-1}$)
The following results have been obtained during the kinetic studies of the reaction:
$2 A + B \rightarrow C + D$
Experiment $[A] / mol \, L^{-1}$ $[B] / mol \, L^{-1}$ Initial rate of formation of $D / mol \, L^{-1} \, min^{-1}$ $I$ $0.1$ $0.1$ $6.0 \times 10^{-3}$ $II$ $0.3$ $0.2$ $7.2 \times 10^{-2}$ $III$ $0.3$ $0.4$ $2.88 \times 10^{-1}$ $IV$ $0.4$ $0.1$ $2.40 \times 10^{-2}$
Determine the rate law and the rate constant for the reaction.
$2 A + B \rightarrow C + D$
| Experiment | $[A] / mol \, L^{-1}$ | $[B] / mol \, L^{-1}$ | Initial rate of formation of $D / mol \, L^{-1} \, min^{-1}$ |
|---|---|---|---|
| $I$ | $0.1$ | $0.1$ | $6.0 \times 10^{-3}$ |
| $II$ | $0.3$ | $0.2$ | $7.2 \times 10^{-2}$ |
| $III$ | $0.3$ | $0.4$ | $2.88 \times 10^{-1}$ |
| $IV$ | $0.4$ | $0.1$ | $2.40 \times 10^{-2}$ |
Determine the rate law and the rate constant for the reaction.
Difficult
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