The empirical formula of a compounds is `CH_(2)O`. 0.25 mole of this compound contains 1 gm hydrogen . The molecular formula of compound is :

Answer

To find the molecular formula of the compound given its empirical formula \( CH_2O \) and the information that 0.25 moles of this compound contains 1 gram of hydrogen, we can follow these steps:

### Step 1: Determine the amount of hydrogen in moles
We know that 1 gram of hydrogen corresponds to 1 mole of hydrogen atoms because the molar mass of hydrogen (H) is approximately 1 g/mol.

### Step 2: Calculate the number of moles of the compound
Since 0.25 moles of the compound contains 1 gram of hydrogen, we can find out how many moles of hydrogen are present in 1 mole of the compound.

\[ \text{Moles of H in 0.25 moles of compound} = 1 \text{ gram of H} = 1 \text{ mole of H} \]

To find the moles of hydrogen in 1 mole of the compound, we can set up a proportion:

\[ \text{Moles of H in 1 mole of compound} = \frac{1 \text{ mole of H}}{0.25 \text{ moles of compound}} = 4 \text{ moles of H} \]

### Step 3: Write the molecular formula
From the empirical formula \( CH_2O \), we can see that it contains 2 moles of hydrogen for every mole of the compound. Now, since we have determined that 1 mole of the compound contains 4 moles of hydrogen, we can express the molecular formula in terms of \( C_xH_yO_z \).

From the empirical formula \( CH_2O \):
- The ratio of \( C:H:O \) in the empirical formula is \( 1:2:1 \).

Since we have determined that the molecular formula must contain 4 moles of hydrogen, we can scale the empirical formula by a factor of 2 (because \( 2 \times 2 = 4 \)):

\[ C_2H_4O_2 \]

### Step 4: Conclusion
Thus, the molecular formula of the compound is \( C_2H_4O_2 \).

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