A 22.60 gram sample of chromium is heated in the presence of excess chlorine. A metal chloride is formed with a mass of 68.83 g. Determine the empirical formula of the metal chloride.

CrCl₃.

Explanation:

From the question given above, the following data were obtained:

Mass of chromium (Cr) = 22.60 g.

Mass of metal chloride = 68.83 g.

Empirical formula =.?

Next, we shall determine the mass of chlorine (Cl) in the metal chloride. This can be obtained as follow:

Mass of chromium (Cr) = 22.60 g.

Mass of metal chloride = 68.83 g.

Mass of chlorine (Cl) =.?

Mass of chlorine (Cl) = (Mass of metal chloride) – (Mass of chromium)

Mass of chlorine (Cl) = 68.83 – 22.60

Mass of chlorine (Cl) = 46.23 g

Finally, we shall determine the empirical formula for the metal chloride as follow:

Cr = 22.60 g.

Cl = 46.23 g

Divide by their molar mass

Cr = 22.60 / 52 = 0.435

Cl = 46.23 / 35.5 = 1.302

Divide by the smallest

Cr = 0.435 /0.435 = 1

Cl = 1.302 /0.435 = 3

The empirical formula for the metal chloride is CrCl₃

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.