The rate constant for the reaction is 0.660 M − 1 ⋅ s − 1 0.660 M−1⋅s−1 at 200 ∘ C. 200 ∘C. A ⟶ products A⟶products If the initial concentration of A A is 0.00440 M, 0.00440 M, what will be the concentration after 865 s?

The concentration of A after 865 seconds is 0.00125 M

Explanation:

The integrated rate law equation for second order reaction follows:

where,

k = rate constant =

t = time taken = 865 second

[A] = concentration of substance after time 't' = ?

= Initial concentration = 0.00440 M

Putting values in above equation, we get:

Hence, the concentration of A after 865 seconds is 0.00125 M

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