Question

What is the empirical and molecular formula of a compound consisting of 27.3?

Answer 1

The empirical formula is BH3. The molar mass of the compound is 27.7 g/mol. The molecular formula is B2H6.

Step-by-step explanation:

The empirical formula of a compound consisting of boron and hydrogen is BH3. The molar mass of the compound is given as 27.7 g/mol. To find the molecular formula, we need to determine the ratio between the empirical formula mass and the molar mass.

The empirical formula mass of BH3 is 13 amu. Therefore, the ratio between the empirical formula mass and the molar mass is 27.7 g/mol divided by 13 amu, which is approximately 2.13.

The ratio tells us that the molecular formula must have twice as many atoms as the empirical formula. So, the molecular formula is B2H6.

Answer 2

To determine the molecular formula of a compound with an empirical formula of BH3 and a molar mass of 27.7 g/mol, calculate the ratio of the compound's molar mass to the molar mass of the empirical formula, which gives a molecular formula of B2H6.

Step-by-step explanation:

The student is asked to determine the molecular formula of a compound given that the empirical formula is BH3 and the molar mass is 27.7 g/mol.

To find the molecular formula, first, calculate the molar mass of the empirical formula. The molar mass of BH3 is the sum of the atomic masses of boron (10.81 g/mol) and three hydrogen atoms (1.01 g/mol each), which equals 13.84 g/mol.

Next, divide the molar mass of the compound by the molar mass of the empirical formula to obtain the ratio: 27.7 g/mol / 13.84 g/mol ≈ 2. This ratio tells us that the molecular formula contains twice as many atoms as the empirical formula, so the molecular formula is B2H6.