A 2 litre container contains 4 moles of `N_(2)O_(5)`. On heating to `100^(@)C, N_(2)O_(5)` undergoes complete dissociation to `NO_(2)` and `O_(2)`. If rate constant for decomposition of `N_(2)O_(5)` is `6.2xx10^(-4)"sec"^(-1)` select the correct statemertns:

Options

A. The mole ratio before and after dissociation is 4:2
B. The time required to complete 40% of reaction is 824 sec
C. `t_(1//2)` of `N_(2)O_(5)` is 1117.7 sec and it is independent of temperature.
D. If volume of container is doubled, the rate of decomposition becomes half of the initial rate

Answer

B, D

Explanation

`4"mole" " "0" "0`
`0 " 8" "2`
a. `4:10=2:5` b. `Kxxt=2.303log((C_(0))/(C_(t)))`
`6.2xx10^(-4)t=2.303log(100/60),t=(2.303xx0.2219)/(6.2xx10^(-4))=0.0824xx10^(4)=824` sec
c. `(t_(1/2))=0.693//(6.2xx10^(-4))=0.11177xx10^(4)=1117.7`