What is first order half life derivation?
1 Answer
Well, let us begin from the rate law... Is the FIRST-order half-life dependent on concentration?
The first-order rate law for the reaction
#A -> B#
is
#r(t) = k[A] = -(d[A])/(dt)# where:
#r(t)# is the rate as a function of time, which we take to be the initial rate in#"M/s"# #k# is the rate constant. What are the units? You should know this.#[A]# is the concentration of a reactant#A# in#"M"# .#(d[A])/(dt)# is the rate of disappearance of reactant#A# , a NEGATIVE value. But the negative sign forces the rate to be positive, fitting for a FORWARD reaction.
By separation of variables:
#-kdt = 1/([A])d[A]#
Integrate on the left from time zero to time
#-kint_(0)^(t)dt = int_([A]_0)^([A])1/([A])d[A]#
#-kt = ln[A] - ln[A]_0#
Therefore, the first-order integrated rate law is:
#color(green)(ln[A] = -kt + ln[A]_0)#
As we should recognize, the half-life is when the concentration drops by half. Hence, we set
#ln0.5[A]_0 = -kt_(1//2) + ln[A]_0#
#ln0.5[A]_0 - ln[A]_0 = -kt_(1//2)#
#ln\frac(0.5cancel([A]_0))(cancel([A]_0)) = -kt_(1//2)#
#-ln0.5 = ln2 = kt_(1//2)#
As a result, the half-life is given by...
#color(blue)(barul|stackrel(" ")(" "t_(1//2) = (ln2)/k" ")|)#