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

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation: