A 2 litre container contains 4 moles of N₂O₅ . On heating to 100°C, N₂O₅   undergoes complete dissociation toNO₂ and O₂ . If rate constant for decomposition of N2O5 is6.2 × 10−4sec−1 , select the correct statements

According to give data, K=6.2 x ${10}^{-4} {\sec }^{-1}$

$\mathrm{K}=\frac{2.303}{\mathrm{t}}\log \left(\frac{\mathrm{a}}{\mathrm{a}-\mathrm{x}}\right)$

$6.2 \mathrm{x} {10}^{-4}=\frac{2.303}{\mathrm{t}}\log \left(\frac{\mathrm{a}}{\mathrm{a}-{\displaystyle \frac{40\mathrm{a}}{100}}}\right)$

$6.2 \mathrm{x} {10}^{-4}=\frac{2.303}{\mathrm{t}}\log \left(\frac{100\mathrm{a}}{60\mathrm{a}}\right)$

$2.2 \mathrm{x} {10}^{-4}=\frac{2.303}{\mathrm{t}}\log \left(5/3\right)$

$\mathrm{t}=\frac{2.303 \mathrm{x} \log \left(1.666\right)}{6.2 \mathrm{x} {10}^{-4}}$

$\mathrm{t}=\frac{2.303\mathrm{x}0.2218\mathrm{x}{10}^4}{0.2}$

$\mathrm{t}=\frac{0.5109}{6.2}\mathrm{x}{10}^4$

$\mathrm{t}=0.0824\mathrm{x}{10}^4$

$\mathrm{t}=0.0824\mathrm{x}{10}^4$

t=824sec

r=K[A]

${\mathrm{r}}^1=\mathrm{k}\left[\frac{\mathrm{nA}}{2\mathrm{A}}\right]$

${\mathrm{r}}^1=\frac{\mathrm{K}}{2}\left[\frac{\mathrm{nA}}{\mathrm{r}}\right]$

${\mathrm{r}}^1=\frac{\mathrm{k}}{2}\left[\mathrm{A}\right]$${\mathrm{r}}^1=\frac{\mathrm{r}}{2}$

If volume of container is doubled the rate of decomposition become half of the initial rate.