Element A has a mass of 0.444 grams and reacts with Element B via a combination reaction. The mass of the product is 0.988 grams. The molar mass of Element A is 111 g/mol and the molar mass of Element B is 68 g/mol. What is the empirical formula of the product.

AB2

Explanation:

The following data were obtained from the question:

Mass of element A = 0.444 g

Molar mass of element A = 111 g/mol

Mass of the compound = 0.988 g

Molar mass of Element B = 68 g/mol

Next, we shall determine the mass of element B. This is shown below:

Mass of element B = Mass of the compound - Mass of Element A

Mass of element B = 0.988 - 0.444

Mass of element B = 0.544 g

Now, we can obtain the empirical formula for the compound formed as follow:

A = 0.444

B = 0.544

Divide by their molar mass.

A = 0.444/111 = 4*10¯³

B = 0.544/68 = 8*10¯³

Divide by the smallest

A = 4*10¯³ / 4*10¯³ = 1

B = 8*10¯³/4*10¯³ = 2

Therefore, the empirical formula for the compound formed is AB2