Test: Study of Compounds – Sulphuric Acid - Class 10 MCQ

The reaction of concentrated sulphuric acid with carbon is an oxidation reaction, where carbon is oxidized to carbon dioxide (CO₂), and sulphuric acid is reduced in the process.

Dilute sulphuric acid is reactive with metals, producing metallic sulphates and hydrogen gas. This property is essential in various chemical processes and reactions involving acids.

When dilute sulphuric acid reacts with metallic carbonates, carbon dioxide (CO₂) is evolved. This is a typical reaction of acids with carbonates, resulting in the formation of a salt, water, and carbon dioxide.

The oxidation of sulphur dioxide to sulphur trioxide occurs at 450^°C in the presence of a catalyst, typically vanadium pentoxide. This temperature is optimal for the reaction to proceed efficiently.

The reaction of sulphur trioxide (SO₃) with concentrated sulphuric acid (H₂SO₄) produces oleum (H₂S₂O7). Oleum is sometimes referred to as pyrosulphuric acid and is an intermediate in the production of sulphuric acid.

Concentrated sulphuric acid's strong dehydrating nature enables it to act as an oxidizing agent. It can oxidize certain substances while simultaneously removing water from them in reactions.

The reaction of sulphuric acid with potassium bicarbonate produces potassium sulfate (K₂SO₄), water (H₂O), and carbon dioxide (CO₂) as byproducts. This reaction illustrates the acid's ability to release gases from carbonates and bicarbonates.

Concentrated sulphuric acid has a high boiling point, which allows it to act as a dehydrating agent. Its strong affinity for water means it can effectively remove water from other compounds during reactions.

When concentrated sulphuric acid is mixed with sodium chloride (NaCl), it produces hydrochloric acid (HCl) and sodium bisulfate (NaHSO₄). This reaction is significant in the laboratory preparation of hydrogen chloride gas.

Sulphuric acid is widely used in the fertilizer industry, particularly in the manufacture of ammonium sulphate [(NH₄)₂SO₄], which is a common nitrogen fertilizer used in agriculture.

When oleum (H₂S₂O₇) is diluted with water, the final product is sulphuric acid (H₂SO₄). This reaction is an important step in producing concentrated sulphuric acid for industrial use.

The contact process begins with the roasting of metallic sulphides in air to produce sulphur dioxide. This step is critical for generating the necessary SO₂ for subsequent reactions in the manufacturing of sulphuric acid.

The chemical formula for oleum is H₂S₂O₇. Oleum is a solution of sulphur trioxide in sulphuric acid and is an important intermediate in the production of sulphuric acid.

The melting point of sulphuric acid is 10.4^°C. This relatively low melting point allows it to remain liquid over a wide range of temperatures.

The reaction between sodium sulfide (Na₂S) and sulphuric acid (H₂SO₄) liberates hydrogen sulfide (H₂S) as a gas. This is a characteristic reaction of metal sulfides with acids.

Sulphuric acid is extensively used in the leaching process to extract metals from their ores. It helps to dissolve metal compounds, allowing for the recovery of pure metals through electrolysis.

The boiling point of sulphuric acid is 338^°C. This high boiling point is one reason why it is used as a dehydrating agent in various chemical reactions.

Vanadium pentoxide acts as a catalyst in the contact process, facilitating the oxidation of sulphur dioxide (SO₂) to sulphur trioxide (SO₃) without being consumed in the reaction.

Sulphuric acid is highly corrosive and can cause severe burns upon contact with skin. It is essential to handle this acid with care, using appropriate protective equipment to prevent injury.

The reaction between dilute sulphuric acid and sodium hydroxide produces sodium bisulfate (NaHSO₄) and water (H₂O). This demonstrates the acid's role in neutralization reactions.