olecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s-1. (a) What is the half-life for this reaction? s (b) If you start with 0.048 M I2 at this temperature, how much will remain after 5.37 s assuming that the iodine atoms do not recombine to form I2? M

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Explanation:

Hello,

In this case, considering the reaction:

Which is first-order with respect to I₂, we can compute the half-life by:

Moreover, since the integrated rate law is:

We can compute the concentration of iodine once 5.37 s have passed:

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it's c. elements are placed in rows based on how may valencies electrons have.