Question

9/15 2 ch₂co₃oh number of c: number of h: number of o: drag these tiles and drop them in the correct blank above 8 6 9 1 7 3 5 10 4 2

Explanation:

Step1: Calculate number of C atoms

In one \( \text{CH}_2\text{CO}_3\text{OH} \), the number of C atoms is 2 (from \( \text{CH}_2 \) and \( \text{CO}_3 \)). For \( 2 \text{CH}_2\text{CO}_3\text{OH} \), we multiply by 2: \( 2\times2 = 4 \)? Wait, no, wait. Wait, formula is \( \text{CH}_2\text{CO}_3\text{OH} \). Let's parse the formula: \( \text{C} \), \( \text{H}_2 \), \( \text{C} \), \( \text{O}_3 \), \( \text{O} \), \( \text{H} \). Wait, no, correct parsing: \( \text{CH}_2\text{CO}_3\text{OH} \) can be written as \( \text{C}_2\text{H}_3\text{O}_4 \)? Wait, no, let's do atom by atom.

For Carbon (C): In one molecule of \( \text{CH}_2\text{CO}_3\text{OH} \), how many C? Let's see: first C, then another C (from \( \text{CO}_3 \))? Wait, no, the formula is \( \text{CH}_2\text{CO}_3\text{OH} \). Let's break it down:

- C: Let's count the C atoms. The formula is \( \text{CH}_2 - \text{CO}_3 - \text{OH} \)? Wait, no, the formula is \( \text{CH}_2\text{CO}_3\text{OH} \). So the atoms:

- C: first C, then the C in \( \text{CO}_3 \)? Wait, no, the formula is \( \text{CH}_2\text{CO}_3\text{OH} \), so the C atoms: let's see, the formula is \( \text{C}_2 \) (because there are two C's: one from \( \text{CH}_2 \), one from \( \text{CO}_3 \))? Wait, no, let's write the formula properly. Let's expand \( \text{CH}_2\text{CO}_3\text{OH} \):

- C: 2 (because \( \text{CH}_2 \) has 1 C, \( \text{CO}_3 \) has 1 C, so total 2 C per molecule)
- H: \( \text{CH}_2 \) has 2 H, \( \text{OH} \) has 1 H, so total 3 H per molecule
- O: \( \text{CO}_3 \) has 3 O, \( \text{OH} \) has 1 O, so total 4 O per molecule

Now, the coefficient is 2 (since it's \( 2 \text{CH}_2\text{CO}_3\text{OH} \)), so we multiply each atom count by 2.

Step2: Number of C atoms

Per molecule: 2 C. With coefficient 2: \( 2 \times 2 = 4 \)? Wait, no, wait: wait, the formula is \( \text{CH}_2\text{CO}_3\text{OH} \). Let's count again:

Wait, maybe I made a mistake. Let's write the formula as \( \text{C}_2\text{H}_3\text{O}_4 \)? Wait, no, let's do it step by step.

First, the formula is \( 2 \times (\text{C} + \text{H}_2 + \text{C} + \text{O}_3 + \text{O} + \text{H}) \)? No, that's not right. Let's use the subscripts.

In the formula \( \text{CH}_2\text{CO}_3\text{OH} \):

- C: The first C (subscript 1, since no number), then the C in \( \text{CO}_3 \) (subscript 1). So total C per molecule: 1 + 1 = 2.
- H: \( \text{H}_2 \) (subscript 2) and \( \text{OH} \) (subscript 1 for H). So total H per molecule: 2 + 1 = 3.
- O: \( \text{CO}_3 \) (subscript 3) and \( \text{OH} \) (subscript 1 for O). So total O per molecule: 3 + 1 = 4.

Now, the coefficient is 2, so we multiply each by 2:

- C: \( 2 \times 2 = 4 \)? Wait, no, wait: the coefficient is 2, so number of C atoms is 2 (molecules) * 2 (C per molecule) = 4? Wait, but the tiles have 4 as an option (the tile with 4). Wait, but let's check again.

Wait, maybe the formula is \( \text{CH}_2\text{CO}_3\text{OH} \) – let's count the C atoms:

First part: \( \text{CH}_2 \) – 1 C.

Second part: \( \text{CO}_3 \) – 1 C.

Third part: \( \text{OH} \) – 0 C.

So total C per molecule: 1 + 1 = 2.

With 2 molecules (coefficient 2), total C: 2 * 2 = 4.

Step3: Number of H atoms

Per molecule: \( \text{CH}_2 \) has 2 H, \( \text{OH} \) has 1 H. So 2 + 1 = 3 H per molecule.

With 2 molecules: 2 * 3 = 6 H.

Step4: Number of O atoms

Per molecule: \( \text{CO}_3 \) has 3 O, \( \text{OH} \) has 1 O. So 3 + 1 = 4 O per molecule.

With 2 molecules: 2 * 4 = 8 O.

Wait, let's verify:

- C: 2 molecules * 2 C/molecule = 4
- H: 2 molecules * 3 H/molecule = 6
- O: 2 molecules * 4 O/molecule = 8

So the numbers are:

Number of C: 4

Number of H: 6

Number of O: 8

Answer:

Number of C: 4
Number of H: 6
Number of O: 8