The rate constant for the reaction is 0.180 M -1.S-1
at 200 C.
A-->products
If the initial concentration of A is 0.00180 M, what will be the
concentration after 535 s?
Given that k = 0.18 M-1s-1
It is rate constant of 2nd order reaction because units of first order reaction rate constant = M-1s-1
For first order recation,
k = [1/t] { 1/ [A]t -1/[A]o} -----Eq (1)
Given that
time t = 535 s
Initial concentration [A]o = 0.0018 M
Final concentration [A]t = ? M
Substitute ll the values in eq (1) ,
k = [1/t] { 1/ [A]t -1/[A]o}
0.18 = [1/535] { 1/[A]t - 1/0.0018 }
On solving,
[A]t = 0.00153 M
Therefore,
concentration after 535 s = 0.00153 M
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