Empirical formula of a compound is `CH_2O`. Its molecular mass is 60. The molecular formula will be

Options

A. `CH_2O`
B. `C_2H_4O_2`
C. `C_3H_6O_3`
D. none of these

Explanation

To find the molecular formula from the empirical formula and the molecular mass, follow these steps:

### Step 1: Determine the Empirical Formula Mass
The empirical formula given is CH₂O. We need to calculate its mass by adding the atomic masses of each element in the formula.

- Carbon (C) has an atomic mass of 12 g/mol.
- Hydrogen (H) has an atomic mass of 1 g/mol. Since there are 2 hydrogen atoms, the total mass contributed by hydrogen is 2 × 1 = 2 g/mol.
- Oxygen (O) has an atomic mass of 16 g/mol.

Now, calculate the empirical formula mass:
\[ \text{Empirical Formula Mass} = \text{mass of C} + \text{mass of H} + \text{mass of O} = 12 + 2 + 16 = 30 \text{ g/mol} \]

### Step 2: Find the Molecular Mass
The molecular mass is given as 60 g/mol.

### Step 3: Calculate the n Factor
The n factor is calculated by dividing the molecular mass by the empirical formula mass:
\[ n = \frac{\text{Molecular Mass}}{\text{Empirical Formula Mass}} = \frac{60}{30} = 2 \]

### Step 4: Determine the Molecular Formula
To find the molecular formula, multiply the subscripts in the empirical formula by the n factor:
- The empirical formula is CH₂O.
- Multiply each subscript by n (which is 2):
- Carbon: \(1 \times 2 = 2\)
- Hydrogen: \(2 \times 2 = 4\)
- Oxygen: \(1 \times 2 = 2\)

Thus, the molecular formula is:
\[ \text{Molecular Formula} = C_2H_4O_2 \]

### Final Answer:
The molecular formula of the compound is \(C_2H_4O_2\).

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