The following reaction descomposes `N_(2)O_(5)rarr 2NO_(2)+(1)/(2)O_(2)`. At a 25 degree centigrade the rate constant of the reaction is `5xx10^(-3)sec^(-1)`. The intial pressure of `N_(2)O_(5)` is 0.2 atm. If total pressure of gaseous mixture becomes 0.35 atm, then calculate the time of decomposition of `N_(2)O_(5)`.

In the reaction 2N_(2)O_(5) rarr 4NO_(2) + O_(2) , initial pressure is 500 atm and rate constant K is 3.38 xx 10^(-5) sec^(-1) . After 10 minutes the final pressure of N_(2)O_(5) is

In the reaction 2N_(2)O_(5) rarr 4NO_(2) + O_(2) , initial pressure is 500 atm and rate constant K is 3.38 xx 10^(-5) sec^(-1) . After 10 minutes the final pressure of N_(2)O_(5) is

N_(2)O_(5(g)) is at a pressure of 0.5 atm. After 100 s the pressure of the decomposition mixture is 0.512 atm. Calculate the rate constant.

In the reaction 2N_2 O_5 rarr 4NO_2 + O_2 , the initial pressure is 500 atm and the rate constant k is 3.38 xx 10^-5 sec^ -1 . After 10 minutes the final pressure of N_2 O_5 is

For the reaction 2N_(2)O_(5) rarr 4NO_(2)+O_(2) rate of reaction and rate constant are 1.02 xx 10^(-4) and 3.4 xx 10^(-5) sec^(-1) respectively. The concentration of N_(2)O_(5) at that time will be

The decomposition of "N"_(2)"O"_(5)(g), i.e.,"N"_(2)"O"_(5)(g)to4"NO"_(2)(g)+"O"_(2)(g) is a first order reaction with a rate constant of 5xx10^(-4)"sec"^(-1)" at "45^(@)C . If intial concentration of "N"_(2)"O"_(5) is 0.25 M, calculate its concentration after 2 min. Also calculate half life for the decomposition of "N"_(2)"O"_(5)(g).

For the reaction N_(2)O_(5) rarr 2NO_(2) + (1)/(2) O_(2) , the rate of disappearance of N_(2)O_(5) is 6.25 xx 10^(-3) "mol L"^(-1) s^(-1) . The rate of formation of NO_(2) and O_(2) will be respectively.