Test: Hydrogen - SSS 2 MCQ

The process is termed a displacement reaction, as more reactive metals displace hydrogen from its compounds like water and dilute acids, leading to the release of hydrogen gas.

During the electrolysis of water, hydrogen gas is collected at the cathode (negative electrode), while oxygen is collected at the anode (positive electrode). This separation is crucial for utilizing both gases.

A redox reaction involves both oxidation (loss of electrons) and reduction (gain of electrons) occurring simultaneously. In the context of hydrogen reactions, it often acts as a reducing agent.

This is a reduction reaction. Hydrogen reduces copper(II) oxide (CuO) to copper metal by removing oxygen from the oxide, demonstrating hydrogen's strong reducing properties.

Hydrogen is primarily used to synthesize ammonia (NH₃) through the Haber process. Ammonia is a key ingredient in fertilizers, which support global food production.

In the Haber process, hydrogen is one of the primary reactants used to synthesize ammonia from nitrogen. This reaction is essential for producing fertilizers that are vital for agriculture.

Catalytic hydrogenation is the process where liquid vegetable oils are treated with hydrogen under pressure in the presence of catalysts like nickel or palladium to produce solid fats, such as margarine.

Hydrogen is highly flammable and burns readily in air or oxygen, producing water vapor. This property makes it a useful fuel but also necessitates careful handling to avoid explosions.

Hydrogen is indeed colorless, odorless, and tasteless. It is also the lightest element, making it much lighter than air.

Metals that are above hydrogen in the activity series are capable of displacing hydrogen from acids, while those below cannot. This series helps predict the outcomes of displacement reactions.

Hydrogen is the most abundant element in the universe, making up about 90% of all matter. It is primarily found in stars, including our Sun, where it plays a crucial role in energy production through nuclear fusion.

Sodium is one of the metals that reacts vigorously with cold water to produce hydrogen gas and sodium hydroxide. This reaction is highly exothermic and can be explosive.

When hydrogen burns in oxygen, it forms water (H₂O). This reaction is highly exothermic and releases a significant amount of energy, making hydrogen a powerful fuel source.

Metals such as aluminum react with hot alkali solutions like sodium hydroxide to produce hydrogen gas. This reaction is often employed in various chemical processes.

The boiling point of hydrogen is -253°C. At this temperature, hydrogen gas can be liquefied, which is important for various applications, including in rocket fuels.

Water gas is primarily composed of hydrogen and carbon monoxide. It is produced by passing steam over hot carbon (coke), and it serves as a significant source of hydrogen in industrial processes.

Liquid hydrogen is significant as a clean fuel in rocket propulsion systems. It provides a high-energy output when burned with oxygen, making it an essential component for space exploration missions.

When hydrogen reacts with chlorine gas, it forms hydrogen chloride (HCl). This reaction can be explosive in bright sunlight, showcasing the reactivity of hydrogen with halogens.

Iron is used as a catalyst in the Haber process, which synthesizes ammonia from nitrogen and hydrogen gas. This process is crucial for producing fertilizers, significantly impacting agricultural productivity.

Henry Cavendish is credited with the discovery of hydrogen as a distinct element in 1766, when he referred to it as "inflammable air." His experiments demonstrated its properties, including the fact that it produces water when burned.