If you start with 0.054 M I2 at this temperature, how much will remain after 5.42 s assuming that the iodine atoms do not recombine to form I2?
sorry this was the info given Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s−1.
To determine how much I2 will remain after 5.42 seconds, we need to calculate the rate of the reaction and use it to determine the decrease in concentration over the given time period.
The rate of the reaction can be expressed as the change in concentration over time (∆[I2]/∆t). However, in this case, since the iodine atoms do not recombine to form I2, the rate will be proportional to the concentration of I2.
Let's assume that the rate constant for this reaction is k.
First, let's find the rate of the reaction at t = 0. This will be equal to k times the initial concentration of I2:
Rate = k * [I2]
At t = 0, the concentration of I2 is 0.054 M. Therefore,
Initial Rate = k * 0.054 M
Next, let's calculate the decrease in concentration (∆[I2]) after 5.42 seconds using the rate of the reaction:
∆[I2] = Rate * ∆t
∆[I2] = (k * 0.054 M) * 5.42 s
Finally, we can calculate the remaining concentration of I2:
[I2] remaining = [I2] initial - ∆[I2]
[I2] remaining = 0.054 M - (k * 0.054 M * 5.42 s)
Please note that we need the value of the rate constant (k) to obtain the exact concentration of I2 remaining after 5.42 seconds.
To determine how much I2 will remain after a given time, we need to use the concept of reaction rate and the rate equation.
First, we need to identify the rate equation for this reaction. Since the iodine atoms do not recombine to form I2, we can assume this is a first-order reaction with respect to I2. This means that the rate of the reaction is proportional to the concentration of I2.
The rate equation for a first-order reaction is given as:
rate = k[I2]
Where rate is the rate of the reaction, k is the rate constant, and [I2] is the concentration of I2.
Since the rate is given as the change in concentration with time, we can integrate this rate equation to find the expression for concentration as a function of time.
∫(d[I2])/[I2] = ∫k dt
Integrating both sides,
ln[I2] = -kt + C
Where ln is the natural logarithm, k is the rate constant, t is the time, and C is the constant of integration.
Now, we can solve for the remaining concentration of I2 after a given time (t) by plugging in the known values.
Given:
Initial concentration [I2]0 = 0.054 M
Time (t) = 5.42 s
Substituting these values into the equation:
ln[I2] = -kt + C
ln[0.054] = -k(5.42) + C
Now, we can consider that "assuming that the iodine atoms do not recombine to form I2" implies that the reaction is irreversible. This condition allows us to calculate the remaining concentration of I2 using the given information.
Next, we need to know the value of the rate constant (k) for this reaction. However, the value of the rate constant depends on the specific reaction and is not provided in the question. Therefore, we cannot directly calculate the remaining concentration of I2 without the value of the rate constant (k).
To find the remaining concentration of I2 after 5.42 seconds, we need the rate constant (k) or other information that can be used to determine it.