A 43.56 gram sample of iron is heated in the presence of excess sulfur. A metal sulfide is formed with a mass of 81.08 g. Determine the empirical formula of the metal sulfide.

Fe2S3

Explanation:

Data obtained from the question include:

Mass of Fe = 43.56g

Mass of metal sulfide = 81.08g

Next we shall determine the mass of sulphur, S in the compound. This is illustrated below:

Mass of S = Mass of metal sulfide – mass of Fe

Mass of S = 81.08 – 43.56 = 37.52g

The empirical formula for the metal sulfide can be obtain as follow:

Fe = 43.56g

S = 37.52g

Divide by their molar mass

Fe = 43.56/56 = 0.7779

S = 37.52/32 = 1.1725

Divide by the smallest

Fe = 0.7779/0.7779 = 1

S = 1.1725/0.7779 = 1.5

Multiply through by 2 to express in whole number

Fe = 1 x 2 = 2

S = 1.5 x 2 = 3

Therefore, the empirical formula for the metal sulfide is Fe2S3

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: