Saved Bookmarks
| 1. |
\( 2 N _{2} O _{5} \longrightarrow 4 NO _{2}+ O _{2} \) if rate of Appearance of NO2 is \( 2 mol L ^{-1} \) find.i) Rate of Reactionii) Rate of Disappearance of \( N _{2} S \) |
|
Answer» \(2N_2O_5 \longrightarrow 4NO_2 + O_2\) Overall rate of reaction r = \(\frac{-1}2 \frac{d[N_2O_5]}{dt}\) \(= +\frac14\frac{d[NO_2]}{dt}\) \(= + \frac{d[O_2]}{dt}\) ∵ Given, rate of appearance of NO2 = \(= \frac{d[NO_2]}{dt} = 2 mol/L\) (i) ∴ rate of reaction r = \(+\frac14\frac{d[NO_2]}{dt}\) \(= \frac14\times2 \) \(= \frac12 mol/L.s\) (ii) rate of disappearance of N2O5 = \(- \frac{d[N_2O_5]}{dt}\) ∵ \(r =\frac{-1}2 \frac{d[N_2O_5]}{dt}\) \(- \frac{d[N_2O_5]}{dt} = 2 \times\frac12\) \(= 1 mol/L.s\) Hence, rate of disappearance of N2O5 is 1 mol/L.s. |
|