In a second-order reaction, the initial concentration of reactant A is 0.20 M, and the rate constant (k) is 0.05 L/mol·s. Calculate the time it takes for [A] to decrease to 0.10 M.

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Topic: Chemistry Posted 1 year ago

In a second-order reaction, the initial concentration of reactant A is 0.20 M, and the rate constant (k) is 0.05 L/mol·s. Calculate the time it takes for [A] to decrease to 0.10 M.

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Koala Tutor

Oct 17, 2023

Koala Ai Support

The second-order reaction can be represented as:

A -> products

The integrated second-order rate equation for this reaction is:

1/[A]t - 1/[A]0 = kt

Where [A]t is the concentration of A at time t, [A]0 is the initial concentration of A, k is the rate constant, and t is the time.

Given that [A]0 = 0.20 M, [A]t = 0.10 M, and k = 0.05 L/mol·s, we can rearrange the equation to solve for t:

1/[A]t - 1/[A]0 = kt

1/0.10 - 1/0.20 = (0.05)t

10 - 5 = (0.05)t

5 = (0.05)t

Divide both sides by 0.05:

5/0.05 = t

100 = t

Therefore, it takes 100 seconds for [A] to decrease to 0.10 M.

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