t75% and t50 % for second order reaction
Answers
second order reaction is a reaction in which rate of reaction depends on the sum of power of reactant.
i.e.
this is the differential equation
the integral equation would be after integrating it from t=0 to t=t i.e. any time during the course of reaction and a= to a i.e. concentration at time t
the equation would be
For t50% half of the reaction has been consumed and half is remaining so putting a=
we get
for t75
the concentration remaining is
i.e. a = a0/4
so t75%=
- A second order reaction is the reaction in which the rate varies with 2nd power of concentration of species
- t = t 50% (t₀.₅₀) corresponds to time when concentration of reactant is 50% of its initial value
- t = t 75%(t₀.₇₅) corresponds to time when concentration of reactant is 75% of its initial value
For a second order reaction, the rate law is given as:
dCₐ/dt = - k Cₐ²
where
dCₐ/dt = rate of disappearance of species 'A'
k = reaction rate constant
Cₐ = concentration of species A at any time t
Now, rearranging the above equation, we get
dCₐ/Cₐ² = - k dt
Integrating the above expression from limits
t = 0 Cₐ = Cₐ₀ (initial concentration of A)
t = t Cₐ = Ca (final concentration of A at time 't')
We get the general expression for concentration profile of A for a second order reaction as follows:
[1/Cₐ] - [1/Cₐ₀] = kt ---------------------------------------------------- equation (1)
Now at t = t 50%
Cₐ = 0.5 Cₐ₀
Replacing Cₐ by 0.5 Cₐ₀ in the above equation, we get
[1/0.5Cₐ₀] - [1/Cₐ₀] = kt₀.₅
⇒[2/Cₐ₀] - [1/Cₐ₀] = kt₀.₅
⇒1/Cₐ₀ = kt₀.₅
t₀.₅ = 1/k Cₐ₀ ------------------------------------------------------------- equation (2)
When t = t 75%
Cₐ= 0.75 Cₐ₀
substituting this value in equation (1)
[1/0.75Cₐ₀] - [1/Cₐ₀] = kt₀.₇₅
⇒(4/3)Cₐ₀ = kt₀.₇₅
⇒t₀.₇₅ = (4/3k)Cₐ₀ ----------------------------------------------------------- equation (3)