A 0.025-g sample of a compound that is composed of B and H, has a molecular mass of about 28 amu and burns spontaneously when exposed to air, producing 0.063 g of `B_2O_3` . Find the molecular formula of the compound

Explanation

To find the molecular formula of the compound composed of boron (B) and hydrogen (H), we will follow these steps:

### Step 1: Determine the moles of \( B_2O_3 \) produced
We know that 0.063 g of \( B_2O_3 \) is produced. First, we need to calculate the molar mass of \( B_2O_3 \).

- Molar mass of \( B_2O_3 \):
- Boron (B): 11 g/mol
- Oxygen (O): 16 g/mol
...