#
**Problem**: 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?

###### FREE Expert Solution

###### FREE Expert Solution

We’re given the following first order reaction:

I_{2}(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]**= initial concentration. We’re being asked to calculate

_{0}**the amount of I**remaining after

_{2}**2.56 s**if we start with

**0.055 M I**.

_{2}This means we have:

**[I _{2}]_{0} = 0.055 M k = 0.271 s^{–1}**

**[I _{2}]_{t} = ?**

**t = 2.56 s**

###### Problem Details

Molecular iodine, I_{2}(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 I_{2} at this temperature, how much will remain after 2.56 s assuming that the iodine atoms do not recombine to form I_{2}?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Integrated Rate Law concept. You can view video lessons to learn Integrated Rate Law Or if you need more Integrated Rate Law practice, you can also practice Integrated Rate Law practice problems .

What is the difficulty of this problem?

Our tutors rated the difficulty of
*
Molecular iodine, I2(g), dissociates into iodine atoms at 62...
*
as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 4 minutes to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hogan's class at LSU.