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
(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
#r(t) = k[A][A] = color(highlight)(k[A]^2 = -(d[A])/(dt)) = (d[C])/(dt)#
Note that despite the fact you have two
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
#kt = 1/[[A]] - 1/[[A]_0]#
Notice how for the half-life,
#kt = 2/[[A]_0] - 1/[[A]_0]#
#= 1/[[A]_0]#
Now, since
#color(blue)(t_"1/2" = 1/(k[A]_0))#
(ii)
Using
#r(t) = k[A][B] = -(d[A])/(dt) = -(d[B])/(dt) = (d[C])/(dt)#
(Clearly if
Notice how we cannot just pick
#(dx)/(dt) = k[A][B]#
#= k([A]_0 - x)([B]_0 - x)#
(since
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