for a second order reaction;
1[A]=1[A0]+kt\dfrac{1}{[A]}= \dfrac{1}{[A_0]}+kt[A]1=[A0]1+kt
Assuming that the rate constant is 977 cMs−1=9.77 Ms−1977\ cMs^{-1} = 9.77\ Ms^{-1}977 cMs−1=9.77 Ms−1
The equation becomes;
1[A]=1[A0]+9.77t\dfrac{1}{[A]}= \dfrac{1}{[A_0]}+9.77t[A]1=[A0]1+9.77t
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