The empirical formula of a compound is `CH_(2)O`. `0.0835` moles of the compound contains `1.0 g` of hydrogen Molecular formula of the compound is

Options

A. (a)`C_(2)H_(12)O_(6)`
B. (b)`C_(5)H_(10)O_(5)`
C. (c )`C_(4)H_(8)O_(8)`
D. (d)`C_(3)H_(6)O_(3)`

Explanation

To find the molecular formula of the compound with the empirical formula \( CH_2O \), we will follow these steps:

### Step 1: Determine the number of moles of hydrogen in the compound
We know that \( 0.0835 \) moles of the compound contains \( 1.0 \) g of hydrogen.

Using the molar mass of hydrogen (approximately \( 1.0 \, \text{g/mol} \)):
\[ \text{Moles of hydrogen} = \frac{\text{mass of hydrogen}}{\text{molar mass of hydrogen}} = \frac{1.0 \, \text{g}}{1.0 \, \text{g/mol}} = 1.0 \, \text{mol} \]

### Step 2: Calculate the number of moles of hydrogen per mole of the compound
Now, we can find out how many moles of hydrogen are present in \( 1 \) mole of the compound:
\[ \text{Moles of hydrogen in 1 mole of compound} = \frac{1.0 \, \text{mol}}{0.0835 \, \text{mol}} \approx 12 \, \text{mol} \]

### Step 3: Relate the number of hydrogen atoms to the empirical formula
The empirical formula \( CH_2O \) contains \( 2 \) hydrogen atoms. If we have \( 12 \) hydrogen atoms in the molecular formula, we can find the ratio:
\[ \text{Ratio} = \frac{12 \, \text{H}}{2 \, \text{H}} = 6 \]

### Step 4: Determine the molecular formula
Since the ratio is \( 6 \), we multiply the subscripts in the empirical formula \( CH_2O \) by \( 6 \):
\[ \text{Molecular formula} = C_{1 \times 6}H_{2 \times 6}O_{1 \times 6} = C_6H_{12}O_6 \]

### Conclusion
The molecular formula of the compound is \( C_6H_{12}O_6 \).

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