Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations of A.
[A](M) | Initial rate (M/s) |
0.15 | 0.018 |
0.30 | 0.073 |
0.60 | 0.293 |
Estimate the value of the rate constant, k. Express your answer using two significant figures.
to get rate constant we need to get order of reaction
for that let us use the general rate law
Rate = K[A}^x where x is the order.
when [A] = 0.15 M and Rate = 0.018 M/s
(1)... 0.018 M/s= K[ 0.15 M ]^x
when [A] = 0.30 M and Rate = 0.073 M/s
0.073 M/s= K[ 0.30 M ]^x
(2)...0.073 M/s= K[2* 0.15 M ]^x
when [A] = 0.60 M and Rate = 0.293 M/s
0.293 M/s= K[ 0.60 M ]^x
(3)... 0.093 M/s= K[ 2* 0.15 M ]^x
On dividing (2)/(1)
we get 4 = [2]^x
so 2^2 = 2^x
x=2
if we divide (3)/(2) also we get
4 = [2]^x
x=2
Thus order of reaction = 2
********************************
rate law will become
Rate = k[A]^2
use any of the three equation to get rate constant K
0.073 M/s= K[ 0.30 M ]^2
K=0.073 M/s/[ 0.30 M ]^2 = 0..81 M^-1 s^-1
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hope it is helpful
Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations...
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