4.24 The experimental data for decomposition of N₂O₅ [2N₂O₅ → 4NO₂ + O₂ ] in gas phase at 318K are given below:

(i) Plot [N2O5 ] against t.

(ii) Find the half-life period for the reaction.

(iii) Draw a graph between log[N2O5 ] and t.

(iv) What is the rate law ?

(v) Calculate the rate constant.

(vi) Calculate the half-life period from k and compare it with (ii).

t/s	0	400	800	1200	1600	2000	2400	2800	3200
102 × [N2O5]/mol L-1	1.63	1.36	1.14	0.93	0.78	0.64	0.53	0.43	0.35

Kindly go through the solution 

$K=A.e^{-Ea/RT}=\left(6.5\times 10^2\right)e^{-26000K/T}$

$\frac{Ea}{8.314}=26000$

Ea = 216.164kJ/mol $\cong$ $$ 216

Reaction rate is used to measure how fast or slow reactions occur per unit time. The rate constant is a proportionality factor that remains constant for every reaction.

Yes, in elementary reactions, order and molecularity can be the same, but this is not always the case because order is an experimental quantity, and molecularity is a theoretical concept.

Reaction Kinetics, also known as chemical kinetics, is the study of the rate of chemical reaction and the factors affecting the reaction rate, such as temperature, concentration, and catalyst.