A 2 litre container contains 4 moles ofN_(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:

A 2 litre container contains 4 moles ofN_(2)O_(5). On heating to 100^(

1.	A 2 litre container contains 4 moles ofN_(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:
Answer» The MOLE ratio before and after dissociation is 4:2 The time REQUIRED to complete 40% of reaction is 824 sec `t_(1//2)` of `N_(2)O_(5)` is 1117.7 sec and it is independent of temperature. If volume of container is doubled, the rate of decomposition becomes halfof the initial rate Solution :`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`