The initial concentration of `N_(2)O_(5)` in the following first order reaction: `N_(2)O_(5)(g) rarr 2NO_(2)(g)+(1)/(2)O_(2)(g)` was `1.24 xx 10^(-2) mol L^(-1)` at `318 K`. The concentration of `N_(2)O_(5)` after `60 min` was `0.20 xx 10^(-2) mol L^(-1)`. Calculate the rate constant of the reaction at `318 K`.

The initial concentration of `N_(2)O_(5)` in the following first order

1.	The initial concentration of `N_(2)O_(5)` in the following first order reaction: `N_(2)O_(5)(g) rarr 2NO_(2)(g)+(1)/(2)O_(2)(g)` was `1.24 xx 10^(-2) mol L^(-1)` at `318 K`. The concentration of `N_(2)O_(5)` after `60 min` was `0.20 xx 10^(-2) mol L^(-1)`. Calculate the rate constant of the reaction at `318 K`.
Answer» For the first order reaction, `k=2.303/t log a/(a-x)` a=`1.24 xx 10^(-2) mol L^(-1), (a-x) = 0.20 xx 10^(-2) mol L^(-1)`, t=60 min `k=2.303/(60min) xx log(1.24 xx 10^(-2) mol L^(-1))/(0.20 xx 10^(-2) mol L^(-1))= 2.303/(60 min)log6.2` `=2.303/(60 min) xx 0.7924 = 0.0304 min^(-1)`

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