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Combine and simplify the chemical equations:
[tex]$
\begin{array}{l}
C ( s ) + \frac{1}{2} O_2 ( g ) \rightarrow CO ( g ) \\
CO ( g ) + \frac{1}{2} O_2 ( g ) \rightarrow CO_2 ( g )
\end{array}
$[/tex]

When forming the final chemical equation, what should you do with CO?

A. Cancel out CO because it appears as a reactant in one intermediate reaction and a product in the other intermediate reaction.
B. Add the two CO molecules together and write them as reactants in the final chemical reaction.
C. Write CO only once as a reactant in the final chemical reaction.
D. Write CO as a reactant and a product in the final chemical reaction.



Answer :

GinnyAnswer
To determine the final chemical equation, we will consider the given intermediate reactions and simplify the overall reaction.

1. The first reaction provided is:
[tex]\[ \text{C (s) + } \frac{1}{2} \text{O}_2 \text{(g) } \rightarrow \text{CO (g)} \][/tex]

2. The second reaction provided is:
[tex]\[ \text{CO (g) + } \frac{1}{2} \text{O}_2 \text{(g) } \rightarrow \text{CO}_2\text{(g)} \][/tex]

To find the overall reaction, we will sum the two reactions. Summing them gives us:

[tex]\[ \text{C (s) + } \frac{1}{2} \text{O}_2 \text{(g) } + \text{CO (g) + } \frac{1}{2} \text{O}_2 \text{(g)} \rightarrow \text{CO (g) + CO}_2\text{(g)} \][/tex]

Next, we notice that CO appears as both a reactant and a product in the overall reaction. Therefore, we can cancel out CO from both sides of the equation. This leaves us with the simplified final reaction:

[tex]\[ \text{C (s) + O}_2 \text{(g)} \rightarrow \text{CO}_2\text{(g)} \][/tex]

Thus, in forming the final chemical equation, we should cancel out CO because it appears as a reactant in one intermediate reaction and a product in the other intermediate reaction.

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