The initial concentration of `N_(2)O_(5)` in the following first order reaction `N_(2)O_(5)(g) to 2NO_(2)(g) + (1)/(2) O_(2)(g)` was `1.24 xx 10^(-2)` mol `L^(-1)` at 318K. The concentration of `N_(2)O_(5)` after 60 mintues was `0.2 xx10^(-2)` mol `L^(-1)`. Calculate the rate constant of the reaction.

Explanation

Data : `[R]_(0) = 1.24 xx 10^(-2) molL^(-1)`
`[R] = 0.2 xx 10^(-2) mol L^(-1)`
t = 60 min
Formula `k = (2.303)/(t) log ""([R]_(0))/([R])`
` k = (2.303)/(60) log (1.24 xx 10^(-2))/(0.2 xx 10^(2))`
`k = (2.303)/(60) xx log 6.2,`
`k = 0.03 min^(-1)`