If the rate constant of a reaction is $0.03 \mathrm{~s}^{-1}$, how much time does it take for $7.2 \mathrm{~mol} \mathrm{~L}^{-1}$ concentration of the reactant to get reduced to $0.9 \mathrm{~mol} \mathrm{~L}^{-1}$ ? (Given: $\log 2=0.301$ )
If the half-life ( $t_{1 / 2}$ ) for a first order reaction is 1 minute, then the time required for $99.9 \%$ completion of the reaction is closest to :
Following data is for a reaction between reactants A and B :
| Rate $$\mathrm{mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$$ |
$$\mathrm{[A]}$$ | $$\mathrm{[B]}$$ |
|---|---|---|
| $$ 2 \times 10^{-3} $$ |
0.1 M | 0.1 M |
| $$ 4 \times 10^{-3} $$ |
0.2 M | 0.1 M |
| $$ 1.6 \times 10^{-2} $$ |
0.2 M | 0.2 M |
$$ \text { The order of the reaction with respect to } \mathrm{A} \text { and } \mathrm{B} \text {, respectively, are } $$
Which of the following plot represents the variation of $$\ln \mathrm{k}$$ versus $$\frac{1}{\mathrm{~T}}$$ in accordance with Arrhenius equation?
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