nitrogen dioxide is a gas commonly found in polluted air. it is produced when nitric oxide in the air reacts with oxygen gas.
consider the following reaction:
4 molecules of nitric oxide (no) react with 2 molecules of oxygen (o₂) to produce some amount of nitrogen dioxide (no₂).
complete the table below.
| chemical element | number of atoms in the reaction |
| ---- | ---- |
| n |
| o |
during this reaction, how many molecules of nitrogen dioxide (no₂) are produced?
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Accepted Answer

# Explanation:
## Step1: Write the balanced chemical equation
The reaction between nitric oxide (NO) and oxygen ($O_2$) to form nitrogen dioxide ($NO_2$) is: $2NO + O_2
ightarrow 2NO_2$.

## Step2: Determine the moles of $NO_2$ produced
From the balanced equation, 2 moles of NO react with 1 mole of $O_2$ to produce 2 moles of $NO_2$. Here, we have 4 molecules of NO (which is $\frac{4}{N_A}$ moles, but we can work with molecules directly using the ratio). The ratio of NO to $NO_2$ is 2:2 (or 1:1). So, 4 molecules of NO will produce 4 molecules of $NO_2$? Wait, no, let's check the oxygen. Wait, the problem says 4 molecules of NO react with 2 molecules of $O_2$. From the balanced equation, 2 molecules of NO react with 1 molecule of $O_2$ to make 2 molecules of $NO_2$. So, 4 molecules of NO would react with 2 molecules of $O_2$ (since 4/2 = 2, and 2/1 = 2). So the ratio is 4 molecules NO : 2 molecules $O_2$ :? molecules $NO_2$. From the equation, 2 NO + $O_2$ → 2 $NO_2$, so scaling up, 4 NO + 2 $O_2$ → 4 $NO_2$. Wait, no, wait the balanced equation is $2NO + O_2 = 2NO_2$. So moles (or molecules) of NO: $O_2$: $NO_2$ is 2:1:2. So if we have 4 molecules of NO, then the moles of $O_2$ needed is 4/2 = 2 molecules (which matches the problem's 2 molecules of $O_2$). Then the moles of $NO_2$ produced is equal to the moles of NO, so 4 molecules? Wait, no, 2 NO gives 2 $NO_2$, so 4 NO gives 4 $NO_2$. Wait, but let's check the oxygen. Each $O_2$ molecule has 2 O atoms. 2 molecules of $O_2$ have 4 O atoms. Each $NO_2$ has 2 O atoms, so 4 $NO_2$ molecules have 8 O atoms? Wait, no, that can't be. Wait, no, the balanced equation: 2 NO (2 N, 2 O) + $O_2$ (2 O) → 2 $NO_2$ (2 N, 4 O). So total O on left: 2 + 2 = 4, on right: 4. Correct. So if we have 4 NO (4 N, 4 O) and 2 $O_2$ (4 O), total O on left: 4 + 4 = 8, N: 4. Then $NO_2$ has 1 N and 2 O per molecule. So to have 4 N, we need 4 $NO_2$ molecules, which would have 8 O atoms. Perfect, that balances. So 4 molecules of NO and 2 molecules of $O_2$ produce 4 molecules of $NO_2$.

Now, for the table:

For N: Each NO has 1 N atom, so 4 NO molecules have 4 N atoms. In the product $NO_2$, each has 1 N, so 4 $NO_2$ molecules have 4 N atoms. So the number of N atoms in the reaction (reactants + products? Wait, no, the table says "Number of atoms in the reaction" – probably total atoms of each element, which should be conserved (Law of Conservation of Mass).

For N: Reactants: 4 NO molecules, each with 1 N: 4*1 = 4 N atoms. Products: 4 $NO_2$ molecules, each with 1 N: 4*1 = 4 N atoms. So total N atoms: 4.

For O: Reactants: 4 NO molecules (4*1 = 4 O) + 2 $O_2$ molecules (2*2 = 4 O) → total O: 4 + 4 = 8. Products: 4 $NO_2$ molecules (4*2 = 8 O). So total O atoms: 8.

But the question also asks "During this reaction, how many molecules of nitrogen dioxide ($NO_2$) are produced?" From the balanced equation and the amounts given (4 molecules NO, 2 molecules $O_2$), we saw that 4 molecules of $NO_2$ are produced.

Wait, let's recheck the balanced equation. The reaction is $2NO + O_2
ightarrow 2NO_2$. So the mole ratio (or molecule ratio) is NO : $O_2$ : $NO_2$ = 2 : 1 : 2.

Given: 4 molecules NO, 2 molecules $O_2$. Let's see the ratio of NO to $O_2$ in given amounts: 4:2 = 2:1, which matches the balanced equation's ratio (2:1). So the reaction goes to completion with these amounts. Then, the amount of $NO_2$ produced is in the ratio 2 (NO) : 2 ($NO_2$), so 4 molecules NO will produce 4 molecules $NO_2$ (since 4/2 = 2, and 2*2 = 4).

So for the table:

- N: total atoms: 4 (from 4 NO)
- O: total atoms: 4 (from 4 NO) + 4 (from 2 $O_2$) = 8

And the number of $NO_2$ molecules produced is 4.

## Step3: Fill the table
For N: 4 atoms.

For O: 8 atoms.

For the number of $NO_2$ molecules: 4.

Wait, but let's confirm the table. The table has "Chemical element" (N and O) and "Number of atoms in the reaction" (total, reactants + products, but since it's conserved, it's the same as reactants or products).

So:

- N: 4 atoms (4 NO molecules, each with 1 N; products have 4 $NO_2$ with 1 N each, so 4)
- O: 4 (from NO) + 4 (from $O_2$) = 8 (products: 4 $NO_2$ with 2 O each: 8)

And the number of $NO_2$ molecules produced is 4.

# Answer:
For the table:
- N: 4
- O: 8

Number of $NO_2$ molecules produced: 4

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QUESTION IMAGE

Question

Explanation:

Step1: Write the balanced chemical equation

Step2: Determine the moles of \(NO_2\) produced

Answer: