The decomposition of nitrogen dioxide 2NO2-->2NO+O2 occurs in a two-step sequence at elevated tempatures. the first step lis NO2--> NO+O. predict a possible second step that, when combined with the first step, gives the complete reaction
To predict a possible second step in the decomposition of nitrogen dioxide (NO2), we need to consider the overall balanced equation and reactants involved.
Step 1: NO2 → NO + O
The balanced equation for the overall reaction is:
2NO2 → 2NO + O2
Since the first step only produces one oxygen molecule (O), the second step needs to incorporate the remaining oxygen molecule. One possible second step could be:
Step 2: 2NO + O2 → 2NO2
Combining the first and second steps, we get the complete reaction:
2NO2 → 2NO + O2
To determine a possible second step in the decomposition reaction of nitrogen dioxide (NO2), we need to consider the conservation of atoms and the products formed in the first step (NO2 → NO + O).
In the first step, one nitrogen atom (N) and two oxygen atoms (O) are involved. The nitrogen atom ends up in the product NO, while one oxygen atom ends up in the product O. Therefore, in the second step, we need to consider how the remaining oxygen atom combines with the nitrogen atom.
Given that we are looking for a possible combination, the most likely reaction is the bonding of the remaining oxygen atom (O) with the nitrogen atom (N) to form a nitrogen oxide compound. The balanced equation for this reaction would be:
NO + O → NO2
This reaction represents the second step of the overall decomposition reaction. Combining the first step (NO2 → NO + O) with the second step (NO + O → NO2) gives us the complete reaction:
2NO2 → 2NO + O2
Thus, the possible second step in the decomposition of nitrogen dioxide is the combination of one nitrogen oxide molecule (NO) with one remaining oxygen atom (O) to form nitrogen dioxide (NO2).
elemental Oxygen, O is highly reactive.
O+O>O2
combine that with the first step