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Determine the molecular formula of the compound.

A compound is used as a gasoline additive. It has a molecular weight of 60.10 atomic mass units and an empirical formula of [tex]\( C_3H_8O \)[/tex].

The molecular formula is [tex]\( C \)[/tex] [tex]\( \square \)[/tex] [tex]\( H \)[/tex] [tex]\( \square \)[/tex] [tex]\( \square \)[/tex].

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To determine the molecular formula of the compound given its molecular weight and empirical formula, we need to follow these steps:

1. Determine the molecular weight of the empirical formula:
- The empirical formula is [tex]\(C_3H_8O\)[/tex].
- The atomic weight of Carbon (C) is 12.01.
- The atomic weight of Hydrogen (H) is 1.01.
- The atomic weight of Oxygen (O) is 16.00.
- Calculate the weight of the empirical formula:
[tex]\[ (3 \times 12.01) + (8 \times 1.01) + (1 \times 16.00) = 60.11 \][/tex]

2. Compare the molecular weight of the compound to the weight of the empirical formula:
- The given molecular weight is 60.10.
- Calculate the ratio of the molecular weight to the empirical formula weight:
[tex]\[ \frac{60.10}{60.11} \approx 1 \][/tex]

3. Determine the molecular formula:
- The ratio is approximately 1, meaning the molecular formula and the empirical formula are the same.
- Hence, the molecular formula is [tex]\(C_3H_8O\)[/tex].

So, the molecular formula of the compound is:
[tex]\[ C_3H_8O \][/tex]

You should select from the drop-down menu:
[tex]\[ C_3H_8O \][/tex]
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