The decomposition of ozone is believed to occur in two steps

O3 <==> O2 + O
O3 + O ---> 2O2

Identify any reaction intermediate. What is the overall reacion?

I got O3 + O3 --> O2 + 2O2

To determine the reaction intermediate and the overall reaction, let's analyze the given information.

The decomposition of ozone (O3) is believed to occur in two steps:

Step 1: O3 <==> O2 + O (1)

Step 2: O3 + O ---> 2O2 (2)

Now, let's examine these steps:

In Step 1, ozone decomposes into oxygen gas (O2) and a free oxygen atom (O) which serves as a reaction intermediate. Notice that Step 1 is a reversible reaction with a double-headed arrow indicating that the reaction can move in both directions.

In Step 2, the oxygen atom (O) from Step 1 reacts with another molecule of ozone (O3), yielding two molecules of oxygen gas (O2). This step is not reversible and represents the consumption of the reaction intermediate (O).

To find the overall reaction, we need to eliminate the intermediate:

To do that, we need to multiply the first equation by 2 so that the number of atoms of oxygen is the same in both equations:

2(O3) <==> 2(O2) + 2(O) (3)

Now, we can add Equation 2 to Equation 3, canceling out the intermediate (O):

2(O3) + (O3) ---> 3(O2) + 2(O2) (4)

Simplifying Equation 4 gives us the overall reaction:

3(O3) ---> 5(O2)

Therefore, the overall reaction for the decomposition of ozone is 3 molecules of ozone (O3) yield 5 molecules of oxygen gas (O2).