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Jason combines the two intermediate steps shown:

[tex]\[
\begin{array}{l}
N_2(g) + O_2(g) \longrightarrow 2 NO(g) \\
2 NO(g) + O_2(g) \longrightarrow 2 NO_2(g)
\end{array}
\][/tex]

Which best describes what Jason should do with the oxygen molecules?

A. Place two of them as products.
B. Place two of them as reactants.
C. Cancel them out because there is one in each equation.
D. Double them because there is one in each equation.


Sagot :

When combining the two intermediate steps of the reactions:

[tex]\[ \begin{array}{l} \text{1)} \ N_2(g) + O_2(g) \longrightarrow 2 \ NO(g) \\ \text{2)} \ 2 \ NO(g) + O_2(g) \longrightarrow 2 \ NO_2(g) \end{array} \][/tex]

we need to carefully account for the oxygen molecules (O[tex]\(_2\)[/tex]) involved in both reactions.

In the first reaction:
[tex]\[ N_2(g) + O_2(g) \longrightarrow 2 \ NO(g) \][/tex]
one molecule of O[tex]\(_2\)[/tex] is a reactant.

In the second reaction:
[tex]\[ 2 \ NO(g) + O_2(g) \longrightarrow 2 \ NO_2(g) \][/tex]
another molecule of O[tex]\(_2\)[/tex] is a reactant.

When combining the reactions, there is no canceling out of oxygen molecules (O[tex]\(_2\)[/tex]) because they are reactants in both steps. Therefore, we must sum the oxygen molecules from both reactions.

Based on the steps above, Jason should account for both O[tex]\(_2\)[/tex] molecules as reactants.

Hence, the correct answer is:
Place two of them as reactants.
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