The integrated rate equations can be fitted with kinetic data to determine the order of a reaction. The integrated rate equations for zero, first and second order reactions are : Zero order : `[Al =-kt+ [A]_0` First order : `log [A] = -(kt)/2.303 + log [A]_0` Second order : `1/([A])=kt+1/[A]_0` These equations can also be used to calculate the halt life periods of different reactions, which give the time during which the concentration of a reactant is reduced to half of its initial concentration, i.e, at time `t_(1//2), [A] = [A]_0//2` Answer the following (1 to 5) question : The decomposition of nitrogen pentoxide : `2N_2O_5(g) rarr 4NO_2(g) + O_2(g)` is a first order reaction. The plot of log `[N_2O_5]` vs time (min) has slope = - 0.01389. The rate constant k is

Options

A. `1.389xx10^-2 mi n^-1`
B. `3.2xx10^-2 mi n^-1`
C. `6.03xx10^-3 mi n^-1`
D. `71.99 mi n^-1`