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Xelga [282]
3 years ago
13

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 initi

al concentration of A A is 0.00440 M, 0.00440 M, what will be the concentration after 865 s?
Chemistry
1 answer:
Irina-Kira [14]3 years ago
5 0

<u>Answer:</u> The concentration of A after 865 seconds is 0.00125 M

<u>Explanation:</u>

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

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