🤓 Based on our data, we think this question is relevant for Professor Strathman's class at IOWA.
We’re given the following first order reaction:
I2(g) → 2 I(g); k = 0.271 s–1
The integrated rate law for a first order reaction is as follows:
where [A]t = concentration at time t, k = rate constant, t = time, [A]0 = initial concentration. We’re being asked to calculate the amount of I2 remaining after 2.56 s if we start with 0.055 M I2.
This means we have:
[I2]0 = 0.055 M k = 0.271 s–1
[I2]t = ? t = 2.56 s
Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s-1 .
If you start with 0.055 M of I2 at this temperature, how much will remain after 2.56 s assuming that the iodine atoms do not recombine to form I2?
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Based on our data, we think this problem is relevant for Professor Strathman's class at IOWA.