Preparation of Sulphide
Sulphides can be manufactured in a variety of ways, including:
Direct Combination: When iron (Fe) and sulphur (S) are combined, they react to produce iron sulphide (FeS), as illustrated in the equation:
Fe(s) + S(s) → FeS(s)
Reduction of sulphate: By lowering the quantity of sulphate, such as in the interaction between magnesium sulphate (MgSO4) and carbon (C), which produces magnesium sulphide (MgS) and carbon monoxide (CO) gas:
MgSO4(s) + 4C(s) → MgS(s) + 4CO(g)
Precipitation of Insoluble Sulphides: Metal ions (M2+) combine with hydrogen sulphide gas (H2S) to generate metal sulphides (MS) and hydrogen ions (H+), as shown in the equation:
M2+ + H2S(g) → MS(s) + 2H + (aq)
Sulphide
Sulphide is a chemical product generated when sulphur reacts with another element, usually a metal. It is frequently found in minerals such as pyrite (fool’s gold) and galena. Sulphides frequently emit unique odours (such as rotten eggs), and some are hazardous. They have a variety of purposes in industry, including mining for metals such as copper and lead. Sulphides also have a role in natural processes such as volcanic gas production and some biological activities.
This article deals with sulphides, their basic properties, formula, structure, reactions and commonly used sulphide compounds.
Table of Content
- What are Sulphides?
- Classes of Sulphides
- Metal Derivatives of Sulphide
- Preparation of Sulphide
- Structure of Sulphides
- Chemical Reactions of Sulphide
- Sulphide, Sulphite and Sulphate
- Sulpfide Applications
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