Question

The decomposition of N₂O₅ takes place according to I order as

2N₂O₅ ----> 4NO₂ + O₂

Calculate :

(a) The rate constant, if instantaneous rate is 1.4 x 10^-6 mol litre^-1 sec^-1 when concentration of N₂O₅ is 0.04 M.

(b) The rate of reaction when concentration of N₂O₅ is 1.20 M.

(c) The concentration of N₂O₅ when the rate of reaction will be 2.45 x 10^-5 mol litre^-1 sec^-1.

Answer 1

(a) Rate = K [N₂O₅] 

R = 14 x 10^-6/ 0.04 = 3.5 x 10^-5 sec^-1

(b) Also rate = K [N₂O₅]

= 3.5 x 10^-5 x 1.20 = 4.2 x 10^-5 mol litre^-1 sec^-1 

(c) Further rate = K [N₂O₅] 

[N₂O₅]  = 2.45 x 10^-5/ 3.5 x 10^-5 = 0.7 mol litre^-1