Final answer:
The products of the combustion of (CH2)3(OH)2 in excess oxygen are likely to be carbon dioxide and water, with the balanced equation being 2 (CH2)3(OH)2 + 9 O2 → 6 CO2 + 6 H2O, assuming complete combustion.
Step-by-step explanation:
We're asked to predict the products of the reaction where a compound with the formula (CH2)3(OH)2 reacts with O2. This description represents a diol, which can be oxidized by oxygen under the right conditions. The oxidation of alcohols typically requires some form of oxidizing agent and controlled conditions. In an open atmosphere, the alcohol would be combusted rather than oxidized in a way that generates aldehydes or acids. Typically, when organic compounds combust, they form carbon dioxide (CO2) and water (H2O). Without specific conditions or catalysts being stated, we would assume combustion occurs.
If the reaction was a simple combustion in excess oxygen, the balanced chemical equation could look like this:
2 (CH2)3(OH)2 + 9 O2 → 6 CO2 + 6 H2O
This assumes complete combustion in an excess of oxygen. In this process, both carbon atoms and hydrogen atoms are fully oxidized to their most oxidized form, which is CO2 and H2O respectively. Remember, the actual outcome would significantly depend on the specific experimental or industrial conditions provided.