Question

For the reaction \[\ce{2N2O5_{(g)} -> 4NO2_{(g)} + O2_{(g)}}\] at 318 K. Calculate the rate of reaction if the rate of disappearance of N₂O_5(g) is 1.4 × 10⁻³ ms⁻¹.

Answer 1

 \[\ce{2N2O5_{(g)} -> 4NO2_{(g)} + O2_{(g)}}\]

`(-"d"["N"_2"O"_5])/"dt" = 1.4 xx 10^-3  "ms"^-1` ...(Given)

Rate of reaction

`(-1)/2 ("d"["N"_2"O"_5])/"dt" = 1/2 xx 1.4 xx 10^-3`

= 0.7 × 10⁻³ ms⁻¹

= 7 × 10⁻⁴ ms⁻¹