Relate the rate of: 1. decomposition of NO2 to the rate of formation of O2 for the following reaction: 2NO2(g)_2NO(g) +O2(g)?

The rate of decomposition of NO2 is directly related to the rate of formation of O2 in the given reaction. This is because the decomposition of NO2 produces O2 as one of the products. As NO2 decomposes to form NO and O2, the rate at which NO2 decomposes will determine the rate at which O2 is formed. Therefore, the rate of decomposition of NO2 is equal to the rate of formation of O2 in this reaction.

The rate of decomposition of NO2 is equal to the rate of formation of O2. This is because the reaction is 1:1, meaning that for every molecule of NO2 that decomposes, one molecule of O2 is formed.

The rate of a reaction can be expressed as the change in concentration of a reactant or product over time. In this case, the rate of decomposition of NO2 can be expressed as:

```
Rate = -Δ[NO2]/Δt
```

where [NO2] is the concentration of NO2 and t is time.

The rate of formation of O2 can be expressed as:

```
Rate = Δ[O2]/Δt
```

where [O2] is the concentration of O2 and t is time.

Since the rate of decomposition of NO2 is equal to the rate of formation of O2, we can write:

```
-Δ[NO2]/Δt = Δ[O2]/Δt
```

This equation can be rearranged to:

```
Δ[O2]/Δ[NO2] = -1
```

This equation shows that the rate of decomposition of NO2 is equal to the negative of the rate of formation of O2. This means that as the concentration of NO2 decreases, the concentration of O2 increases at the same rate.

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