Answer :
Sure, let's go through the intermediate steps and see how we should handle the oxygen molecules:
1. First Intermediate Step:
[tex]\[ N_2(g) + O_2(g) \longrightarrow 2 NO(g) \][/tex]
This equation shows that nitrogen gas (N₂) reacts with one molecule of oxygen gas (O₂) to produce two molecules of nitrogen monoxide (NO).
2. Second Intermediate Step:
[tex]\[ 2 NO(g) + O_2(g) \longrightarrow 2 NO_2(g) \][/tex]
This equation shows that two molecules of nitrogen monoxide (NO) react with one molecule of oxygen gas (O₂) to produce two molecules of nitrogen dioxide (NO₂).
When combining these two intermediate steps, we want to find the overall balanced equation that summarizes the entire reaction process. Here are the steps:
- First, list all reactants and products from both steps:
- From the first step, the reactants are [tex]\(N_2(g)\)[/tex] and [tex]\(O_2(g)\)[/tex], and the products are [tex]\(2 NO(g)\)[/tex].
- From the second step, the reactants are [tex]\(2 NO(g)\)[/tex] and [tex]\(O_2(g)\)[/tex], and the products are [tex]\(2 NO_2(g)\)[/tex].
- Next, align the two reactions and look for substances that appear on both sides, which could be canceled out if they are intermediates (i.e., produced in one step and consumed in the next):
[tex]\[ N_2(g) + O_2(g) \longrightarrow 2 NO(g) \][/tex]
[tex]\[ 2 NO(g) + O_2(g) \longrightarrow 2 NO_2(g) \][/tex]
- Here, we notice that [tex]\(2 NO(g)\)[/tex] produced in the first reaction is used up as a reactant in the second reaction.
- Therefore, we can cancel out [tex]\(2 NO(g)\)[/tex], as it does not appear in the overall balanced equation. What remains is:
[tex]\[ N_2(g) + O_2(g) + O_2(g) \longrightarrow 2 NO_2(g) \][/tex]
Simplifying this, we get:
[tex]\[ N_2(g) + 2 O_2(g) \longrightarrow 2 NO_2(g) \][/tex]
As a result, Jason should cancel out the oxygen molecules that appear in both intermediate steps, as there is one in each equation. Thus, the best description of what Jason should do with the oxygen molecules is:
Cancel them out because there is one in each equation.
1. First Intermediate Step:
[tex]\[ N_2(g) + O_2(g) \longrightarrow 2 NO(g) \][/tex]
This equation shows that nitrogen gas (N₂) reacts with one molecule of oxygen gas (O₂) to produce two molecules of nitrogen monoxide (NO).
2. Second Intermediate Step:
[tex]\[ 2 NO(g) + O_2(g) \longrightarrow 2 NO_2(g) \][/tex]
This equation shows that two molecules of nitrogen monoxide (NO) react with one molecule of oxygen gas (O₂) to produce two molecules of nitrogen dioxide (NO₂).
When combining these two intermediate steps, we want to find the overall balanced equation that summarizes the entire reaction process. Here are the steps:
- First, list all reactants and products from both steps:
- From the first step, the reactants are [tex]\(N_2(g)\)[/tex] and [tex]\(O_2(g)\)[/tex], and the products are [tex]\(2 NO(g)\)[/tex].
- From the second step, the reactants are [tex]\(2 NO(g)\)[/tex] and [tex]\(O_2(g)\)[/tex], and the products are [tex]\(2 NO_2(g)\)[/tex].
- Next, align the two reactions and look for substances that appear on both sides, which could be canceled out if they are intermediates (i.e., produced in one step and consumed in the next):
[tex]\[ N_2(g) + O_2(g) \longrightarrow 2 NO(g) \][/tex]
[tex]\[ 2 NO(g) + O_2(g) \longrightarrow 2 NO_2(g) \][/tex]
- Here, we notice that [tex]\(2 NO(g)\)[/tex] produced in the first reaction is used up as a reactant in the second reaction.
- Therefore, we can cancel out [tex]\(2 NO(g)\)[/tex], as it does not appear in the overall balanced equation. What remains is:
[tex]\[ N_2(g) + O_2(g) + O_2(g) \longrightarrow 2 NO_2(g) \][/tex]
Simplifying this, we get:
[tex]\[ N_2(g) + 2 O_2(g) \longrightarrow 2 NO_2(g) \][/tex]
As a result, Jason should cancel out the oxygen molecules that appear in both intermediate steps, as there is one in each equation. Thus, the best description of what Jason should do with the oxygen molecules is:
Cancel them out because there is one in each equation.
