Discussion Forum



1)

For the reaction 2N2O5 → 4NO2 + O2, rate and rate constant are 1.02 x 10-4 mol lit-1 sec-1 and 3.4 x 10-5 sec-1 respectively then concentration of N2O5, at that time will be


A) 1.732 M

B) 3 M

C) $3.4\times10^{5}$

D) $1.02\times10^{-4}$

Answer:

Option B

Explanation:

2N2O5 → 4NO2 + O2

from the unit of rate constant it is clear that the reaction follow first order kinetics. Hence by rate law equation

r = k [N2O5]  where r = 1.02 x 10-4, k = 3.4 x 10-5

1.02 x 10-4 = 3.4 x 10-5 [N2O5]  

[N2O5] = 3M