The experiment data for the decompoistion of nitrogen pentoxide in the gaseous phase at `218 K` are as follows: `2N_(2)O_(5)(g) rarr 4NO_(2)(g) + O_(2)(g)`

Calculating the rates of reaction at the time given above (assuming that the rate remains constant during the intervals given). Also find the out the following:
(a) Rate law expresison
(b) Rate constant
(c ) Order of reaction

Explanation

Since the value of `k` comes out to be nearly constant for the expresison rate`//N_(2)O_(5)`, this shows that the rate law expresison is
Rate `= k[N_(2)O_(5)]`
Mean value of `k = 4.96 xx 10^(-4) s^(-1)`