At a certain temperature this reaction follows first-order Kinetics with a rate constant of 0.0660

Chemistry

1 answer:

Juli2301 [7.4K]2 years ago

3 0

Answer:

After 26.0s, the concentration of HI decreases from 0.310M to 0.0558M.

Explanation:

Based on the reaction of the problem, you have as general kinetic law for a first-order reaction:

ln[HI] = -kt + ln [HI]₀

<em>Where [HI] is actual concentration after time t, </em>

<em>k is rate constant </em>

<em>and [HI]₀ is initial concentration of the reactant. </em>

Initial concentration of HI is 0.310M,

K is 0.0660s⁻¹,

And the actual concentration is 0.0558M:

ln[HI] = -kt + ln [HI]₀

ln[0.0558M] = -0.0660s⁻¹*t + ln [ 0.310M]

-1.7148 = -0.0660s⁻¹*t

26.0s = t

<h3>After 26.0s, the concentration of HI decreases from 0.310M to 0.0558M</h3>

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