Sulfur and Its Compounds
Chemistry ⇒ Chemistry of Non-metals and Their Compounds
Sulfur and Its Compounds starts at 9 and continues till grade 12.
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A sample of pyrite (FeS2) weighing 11.2 g is roasted in air to produce sulfur dioxide (SO2) and iron(III) oxide (Fe2O3). Write the balanced chemical equation for the reaction. Calculate the mass of SO2 produced, assuming complete conversion. (Atomic masses: Fe = 56, S = 32, O = 16)
A solution contains both sulfate (SO42−) and sulfide (S2−) ions. Describe a stepwise procedure to distinguish and confirm the presence of each ion using chemical tests. Include the chemical equations for the reactions involved.
Describe the test for the presence of sulfite ions (SO32−) in a solution. Explain the chemical principle behind the test and write the relevant chemical equation.
Explain the industrial process used for the manufacture of sulfuric acid, highlighting the role of catalysts and the importance of temperature control. Write all the relevant chemical equations involved in the process.
Sulfur dioxide (SO2) is a common air pollutant. Describe the chemical reaction that occurs when SO2 is dissolved in water, and explain the environmental impact of this reaction. Write the balanced chemical equation and discuss how this process contributes to acid rain formation.
Compare and contrast the chemical properties of sulfur and oxygen.
Describe the laboratory preparation of hydrogen sulfide (H2S) gas.
Describe the physical properties of sulfur.
Describe the test for the presence of sulfide ions (S2−) in a solution.
Discuss the environmental impact of sulfur dioxide emissions.
Explain the importance of sulfur compounds in biological systems.
Explain the process of the Frasch method for extracting sulfur.
Explain the role of sulfur dioxide (SO2) in the contact process for the manufacture of sulfuric acid.
Explain why sulfuric acid is called the 'king of chemicals'.
Write a short note on the allotropes of sulfur.
