To determine the appearance of oxygen in the final chemical equation, let's first look at the given intermediate chemical equations:
1. [tex]\( C(s) + \frac{1}{2} O_2(g) \rightarrow CO(g) \)[/tex]
2. [tex]\( CO(g) + \frac{1}{2} O_2(g) \rightarrow CO_2(g) \)[/tex]
These two equations can be combined to obtain the overall reaction. Here's the step-by-step combination process:
### Step 1: Write down both equations:
[tex]\[
\begin{array}{l}
1. \ C(s) + \frac{1}{2} O_2(g) \rightarrow CO(g) \\
2. \ CO(g) + \frac{1}{2} O_2(g) \rightarrow CO_2(g)
\end{array}
\][/tex]
### Step 2: Combine the two equations:
When combining, we add the reactants together and add the products together. This results in the following equation:
[tex]\[
C(s) + \frac{1}{2} O_2(g) + CO(g) + \frac{1}{2} O_2(g) \rightarrow CO(g) + CO_2(g)
\][/tex]
### Step 3: Simplify the combined equation:
To simplify, notice that [tex]\( CO(g) \)[/tex] appears on both sides of the reaction. Therefore, we can cancel it out:
[tex]\[
C(s) + \frac{1}{2} O_2(g) + \frac{1}{2} O_2(g) \rightarrow CO_2(g)
\][/tex]
Now, combine the oxygen terms on the reactant side:
[tex]\[
C(s) + 1 O_2(g) \rightarrow CO_2(g)
\][/tex]
### Final Equation:
The simplified overall reaction is:
[tex]\[
C(s) + O_2(g) \rightarrow CO_2(g)
\][/tex]
From the final equation, it is clear that [tex]\( O_2(g) \)[/tex] appears as a reactant.
### Conclusion:
Oxygen, [tex]\( O_2(g) \)[/tex], appears as a reactant in the final chemical equation.
Therefore, the answer is:
[tex]\[ \boxed{O_2(g) \text{ as a reactant}} \][/tex]
