Aluminum And Silver Sulfide

Background of reaction by Chu C. 1st Period

All about Aluminum

Atomic Number: 13

Atomic Weight: 26.9815386

Melting Point: 933.437 K (660.323°C or 1220.581°F)

Boiling Point: 2792 K (2519°C or 4566°F)

Density: 2.70 grams per cubic centimeter

Phase at Room Temperature: Solid

Element Classification: Metal

Period Number: 3 Group Number: 13 Group Name: none

Although aluminum is the most abundant metal in the earth's crust, it is never found free in nature. All of the earth's aluminum has combined with other elements to form compounds. Two of the most common compounds are alum, such as potassium aluminum sulfate (KAl(SO4)2·12H2O), and aluminum oxide (Al2O3). About 8.2% of the earth's crust is composed of aluminum.

Silver Sulfide

Silver sulfide is insoluble in all solvents, but is degraded by strong acids. Silver sulfide features a covalent bond, as it is made up of silver and sulfur. It is a component of classical qualitative inorganic analysis.


Chemical formula: Ag2S

Molar mass: 247.80 g

Appearance: Grayish-black crystal

Odor: Odorless

Melting point: 836 °C

Solubility: Soluble in aq. HCN, aq. citric acid with KNO3 Insoluble in acids, alkalies, aqueous ammoniums

Solving Stoichiometry Problem, this is how you solve this reaction step by step

Aluminum and Silver Sulfide

1st step: Name the type of the reaction

Single Replacement

2nd Step: Balanced Equation

2Al + 3Ag₂S → Al₂S₃ + 6Ag

3rd step: IUPAC name for each reactant and product

Aluminum + Silver Sulfide → Aluminum Sulfide + Silver

4th step: Name the molar mass for each reactant and product

Al: 26.982 g/mole + Ag₂S: 107.868*2+32.066=247.802 g/mole → Al₂S₃: 26.982*2+32.066*3=150.162 g/mole + Ag: 107.868 g/mole

5th step: Mole to mole conversions

6th step: Mass to mass conversions

7th step: Limiting and excess reactant

8th step: Theoretical yield

9th step: Percent yield

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