Question

The decomposition of N₂O_5(g) at 320K according to the following equation follows first order reaction:

`N_2O_(5(g))->2NO_(2(g))+1/2O_(2(g))`

The initial concentration of N₂O_5(g) is 1.24 x 10^-2 mol. L-1 and after 60 minutes 0.20x10^-2 molL^-1. Calculate the rate constant of the reaction at 320K.

Answer 1

Data: `N_2O_(5(g))->2NO_(2(g))+1/2O_2`

`[N_2O_5][email protected]=1.24xx10^-2molL^-1`

`[N_2O_5]_t=0.20xx10^-2molL^-1`

k=?   t=60min

Solution : 

`k=2.303/t log""([N_2O_5])/([N_2O_5])`

`k=2.303/60log""((1.24xx10^-2))/((0.2xx10^-2))`

k=0.0383x0.7924

k= 0.303min^-1