How do I answer this question?
The average rate of disappearance of ozone in the reaction 2O3 --> 3O2 is found to be 8.12 x 10^-3 molecules over 15 seconds. What is the rate of appearance of O2 during this interval?
It must be 1.5x that of ozone rate.
To find the rate of appearance of O2 during the given interval, we need to use the stoichiometry of the reaction.
The balanced chemical equation for the reaction is:
2O3 --> 3O2
From the stoichiometry, we can see that for every 2 molecules of O3 that disappear, 3 molecules of O2 are formed.
First, let's calculate the moles of O3 that disappear during the given interval:
Moles of O3 = (rate of disappearance of O3) * (time interval)
Moles of O3 = (8.12 x 10^-3 molecules) * (15 seconds)
Next, we can use the stoichiometry to determine the moles of O2 formed:
Moles of O2 = (moles of O3) * (3 moles of O2 / 2 moles of O3)
Finally, we can calculate the rate of appearance of O2:
Rate of appearance of O2 = (moles of O2) / (time interval)
To answer this question, we need to find the rate of appearance of O2 during the given interval.
The reaction given is:
2O3 --> 3O2
We are given that the average rate of disappearance of ozone (O3) is 8.12 x 10^-3 molecules over 15 seconds.
Now, we can use stoichiometry to find the rate of appearance of O2.
From the balanced equation, we can see that for every 2 molecules of ozone (O3) that disappear, 3 molecules of oxygen gas (O2) appear.
So, the rate of appearance of O2 is directly proportional to the rate of disappearance of O3.
Using this information, we can set up a ratio to find the rate of appearance of O2:
(rate of appearance of O2) / (rate of disappearance of O3) = (coefficient of O2) / (coefficient of O3)
Substituting the given values:
(rate of appearance of O2) / (8.12 x 10^-3 molecules) = 3 / 2
Now, we can solve for the rate of appearance of O2:
(rate of appearance of O2) = (8.12 x 10^-3 molecules) * (3 / 2)
(rate of appearance of O2) = (8.12 x 10^-3 molecules) * (1.5)
(rate of appearance of O2) = 1.218 x 10^-2 molecules
Therefore, the rate of appearance of O2 during this interval is approximately 1.218 x 10^-2 molecules.