The empricial formula of a compound is `CH_(2)O`. Its molecular weight is 120. The molecular formula of the compound is

Options

A. `C_(3)H_(6)O_(3)`
B. `C_(4)H_(8)O_(4)`
C. `C_(2)H_(4)O_(2)`
D. `C_(6)H_(12)O_(6)`

Answer

To find the molecular formula of the compound given its empirical formula and molecular weight, follow these steps:

### Step 1: Calculate the Empirical Formula Mass
The empirical formula is \( CH_2O \). To find the empirical formula mass, we need to sum the atomic masses of each element in the formula:

- Carbon (C): 1 atom × 12 g/mol = 12 g/mol
- Hydrogen (H): 2 atoms × 1 g/mol = 2 g/mol
- Oxygen (O): 1 atom × 16 g/mol = 16 g/mol

Now, add these values together:

\[ \text{Empirical Formula Mass} = 12 + 2 + 16 = 30 \text{ g/mol} \]

### Step 2: Determine the Value of \( n \)
The value of \( n \) is determined by the ratio of the molecular weight to the empirical formula mass. Given that the molecular weight is 120 g/mol, we can calculate \( n \):

\[ n = \frac{\text{Molecular Weight}}{\text{Empirical Formula Mass}} = \frac{120}{30} = 4 \]

### Step 3: Calculate the Molecular Formula
To find the molecular formula, multiply each subscript in the empirical formula by \( n \):

\[ \text{Molecular Formula} = (CH_2O) \times n = (CH_2O) \times 4 = C_{4}H_{8}O_{4} \]

Thus, the molecular formula of the compound is \( C_{4}H_{8}O_{4} \).

### Final Answer
The molecular formula of the compound is \( C_{4}H_{8}O_{4} \).

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