What is the derivation for the half life of a second order reaction with: (i) equal concentration of reactants for the reaction 2A→product (ii) unequal concentration of reactants for the reaction A+B→product?

1 Answer
Oct 18, 2015

(i)

Only through assuming that each reaction is an elementary reaction do we have

#A + A=> C#

With equal amounts of two disappearing reactants, and calling the appearing product #C#, you have the rate law:

#r(t) = k[A][A] = color(highlight)(k[A]^2 = -(d[A])/(dt)) = (d[C])/(dt)#

Note that despite the fact you have two #A# reactants, you use the stoichiometric coefficient #\mathbf1#, not #2#, because #A# is reacting with itself. It is not two #A# reactants reacting with a #B# reactant.

What we can do is a separation of variables:

#kdt = -1/([A]^2) d[A]#

Then, you can integrate each side with respect to the variable in question.

#int_(t_0)^(t) kdt = int_([A]_0)^([A]) 1/([A]^2) d[A]#

Where #X_0# means "initial #X#". Assuming #t_0 = 0#, we get:

#kt = 1/[[A]] - 1/[[A]_0]#

Notice how for the half-life, #[A] = [A]_0/2#. Thus:

#kt = 2/[[A]_0] - 1/[[A]_0]#

#= 1/[[A]_0]#

Now, since #[A] = [A]_0/2#, #t = t_"1/2"# and we have:

#color(blue)(t_"1/2" = 1/(k[A]_0))#

(ii)

Using #[A]_0 ne [B]_0#, we get a second order reaction of two first-order components #A# and #B#:

#r(t) = k[A][B] = -(d[A])/(dt) = -(d[B])/(dt) = (d[C])/(dt)#

(Clearly if #A = B#, then we are just doing (i).)

Notice how we cannot just pick #[A]# and call it good. We have to consider both. When the concentrations of both compounds decrease, they decrease by an unknown amount, #x#, so we have:

#(dx)/(dt) = k[A][B]#

#= k([A]_0 - x)([B]_0 - x)#

(since #x = [A]_0 - [A] = [B]_0 - [B]#, #x# increases as #[A]# and #[B]# decrease, so #(dx)/(dt) > 0#)

Using separation of variables again, we have:

#int_(t_0)^t kdt = int_(0)^x 1/[([A]_0 - x)([B]_0 - x)] dx#

With this, we need to use partial fractions to integrate the right side. In the interest of time (and partial fractions is not the focus here):

#= 1/([B]_0 - [A]_0) [ln([A]_0/([A]_0 - x)) - ln([B]_0/([B]_0 - x))]#

Using the rules for logarithms, we get:

#kt = 1/([B]_0 - [A]_0) ln(([A]_0)/([A]_0 - x)*([B]_0 - x)/([B]_0))#

#= 1/([B]_0 - [A]_0) ln(([A]_0)/([A])*([B])/([B]_0))#

#= 1/([B]_0 - [A]_0) ln(([B][A]_0)/([A][B]_0))#

#k([B]_0 - [A]_0)t = ln(([B][A]_0)/([A][B]_0))#

#color(blue)(t = ln(([B][A]_0)/([A][B]_0))/(k([B]_0 - [A]_0)))#

Even though we are doing half-life, we don't know their half-lives, so we can't assume that #[A] = [A]_0/2# or that #[B] = [B]_0/2#. So there is no general equation for the half-life for #[A]_0 ne [B]_0#!