The rate constant for this second‑order reaction is 0.990 M − 1 ⋅ s − 1 0.990 M−1⋅s−1 at 300 ∘ C. 300 ∘C. A ⟶ products A⟶products How long, in seconds, would it take for the concentration of A A to decrease from 0.650 M 0.650 M to 0.380 M?

Answer : The time taken would be, 1.10 s

Explanation :

The integrated rate law equation for second order reaction follows:

where,

k = rate constant =

t = time taken  = ?

[A] = concentration of substance after time 't' = 0.380 M

= Initial concentration = 0.650 M

Now put all the given values in above equation, we get:

Hence, the time taken would be, 1.10 s

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