Question

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?

Answer 1

Answer: The concentration of A after 865 seconds is 0.00125 M

Explanation:

The integrated rate law equation for second order reaction follows:

$k=\frac{1}{t}\left (\frac{1}{[A]}-\frac{1}{[A]_o}\right)$

where,

k = rate constant = $0.660M^{-1}s^{-1}$

t = time taken = 865 second

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

$[A]_o$ = Initial concentration = 0.00440 M

Putting values in above equation, we get:

$0.660=\frac{1}{865}\left (\frac{1}{[A]}-\frac{1}{(0.00440)}\right)$

$[A]=0.00125M$

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