Question

(a) From the differential rate equation given below, write a balanced equation for the reaction involved. 1 d[N o,) i d[NO] d[0] N2011 2 2 dt 4 dt dt rate (b) Given, rate = k[NO2]2[Cl2], by what factor does the rate increase of each of the following changes occurs. i. (NO2) is tripled. ii. [NO2] and [Cl2] are doubled [4M]

Answer 1

We are given an equation that shows the differential rate change of the reaction and it is given as

$-\frac{1}{2}\frac{d}{dt}\lbrack N_2O_5\rbrack=\frac{1}{4}\frac{d}{dt}\lbrack NO_2\rbrack=\frac{d}{dt}\lbrack O_2\rbrack$

This depicts the decomposition reaction of N₂O₅. The forward reaction (product) carries a positive sign while the backward reaction or (reactant) carries a negative sign.

We can as well integrate this, but for the sake of simplicity, the equation of reaction is given as

$2N_2O_5\rightleftarrows4NO_2+O_2$