Chemical Kinetics

A certain reaction A + B → Product is first-order w.r.t. each reactant with k = 5.0 x 10-3 M-1s-1. Calculate the concentration of A remaining after 100 s if the initial concentration of A was 0.1 M and that of B was 6.0 M. State any approximation made in obtaining your result.

4 Answers

Rudra Sen ·

.06 mole

Anurag Ghosh ·

Dada first see whether my approach is correct or not......
-d[A]/dt=k[A] (As the reaction is first order w.r.t A and B is present in excess)
Given,the initial concentration of A is 0.1M.Let the final concentration be xM.
∫d[A]/[A]=-∫k.dt (Integration limit for [A] is from 0.1 to x and integration limit for time is from 0 to 100 secs)
After integrating we get,
[x]=10^-3/2........whether this is correct????

Bitan Chakraborty ·

Since [B] = 6.0, we can consider that its concentration remains constant throughout.
Thus, rate = k[A][B] = 6k[A] = k /[A]
where, k / ( = 6k ) is the new constant and reaction under this condition is supposed to follow 1st order kinetics.
k / = 2.303t log (aa-x)
Now putting in the values we have,
aa-x = 20
So that (a-x) = 0.005 M

Anurag Ghosh · do i relate it with solvolysis....plz explain dada????

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