Final answer:
C₈H₁₆(g) + 2O₂(g) -----> CO₂(g) + 2H₂O(g) The oxidation state of carbon in the reactant is -4, and the oxidation state of carbon in the products is +4. The oxidation state of carbon in the reactant C₈H₁₆ is typically -4, and in the products CO₂, it is +4.
Step-by-step explanation:
To determine the oxidation state of carbon in the reactant C₈H₁₆ and in the products of the given chemical reaction, we need to apply the oxidation state rules. In hydrocarbons, like the reactant C₈H₁₆ , carbon typically has an oxidation state of -4 since each hydrogen contributes +1 and carbon tends to form four bonds.
For the products, in carbon dioxide (CO₂), the oxidation state of carbon is +4 because oxygen is more electronegative and assigned an oxidation number of -2, making the total of each CO₂ molecule zero.
It's important to note that while the equation provided in the question appears unbalanced, the oxidation states can still be determined as described for illustration purposes. Also, the rule of thumb is that the oxidation state in elemental form, like carbon as C(s), is always zero.