For the reaction `2N_(2)O_(5)(g) to 4NO_(2) (g) + O_(2)(g)` , the rate of formation of `NO_(2)(g) ` is `2.8 xx 10^(-3) Ms^(-1)` . Calculate the rate of disapperance of `N_(2)O_(5)(g)`.

Explanation

`2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g)`
Rate of formation `(R_(f)) = (Delta[NO_(2)])/(Deltat) = 2.8 xx 10^(-3) ` M/s
Rate of disapperance of `N_(2)O_(5)(g) = (Delta[N_(2)O_(5)])/(Deltat) = ?`
Rate of reaction = `(1)/(2) (Delta[N_(2)O_(5)])/(Deltat) = (1)/(4) (Delta[NO_(2)])/(Deltat)`
`(Delta[N_(2)O_(5)])/(Deltat) = (2)/(4) xx (Delta[NO_(2)])/(Deltat) = (1)/(2) xx 2.8 xx 10^(-3)` M/s
`(Delta[N_(2)O_(5)])/(Deltat) = 1.4 xx 10^(-3) ` M/s