Hydrogen and Its Compounds

Chemistry ⇒ Chemistry of Non-metals and Their Compounds

Hydrogen and Its Compounds starts at 8 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Hydrogen and Its Compounds. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 10

Describe the laboratory preparation of hydrogen gas using zinc and dilute hydrochloric acid. Write the chemical equation involved.

Describe the physical properties of hydrogen gas.

Describe the structure and properties of water as a compound of hydrogen.

Discuss the importance of heavy water (D₂O) and its uses.

Discuss the role of hydrogen in the hydrogenation of vegetable oils.

Explain the difference between ortho-hydrogen and para-hydrogen.

Explain why hydrogen is considered a clean fuel. What are the challenges associated with its use as a fuel?

Explain why hydrogen is placed in Group 1 of the periodic table, but also has similarities with Group 17 elements.

What are the main uses of hydrogen in industry and daily life?

Write a short note on the industrial preparation of hydrogen by the electrolysis of water.

A sample of water is electrolyzed, producing 224 mL of hydrogen gas at STP. Calculate the mass of water decomposed and the volume of oxygen gas produced. (Molar mass of H₂O = 18 g mol^-1, 1 mole of gas at STP = 22.4 L)

Calculate the amount of heat required to convert 36 g of ice at 0°C to steam at 100°C. (Specific heat of water = 4.18 J g^-1 K^-1, latent heat of fusion = 334 J g^-1, latent heat of vaporization = 2260 J g^-1)

Describe the structure of the water molecule and explain, using the concept of hydrogen bonding, why water has a higher boiling point than hydrogen sulfide (H₂S).

Explain, with equations, how hydrogen acts both as a reducing agent and as an oxidizing agent. Give one example of each and describe the changes in oxidation states involved.

Hydrogen can be prepared in the laboratory by the reaction of dilute hydrochloric acid with zinc. Write the balanced chemical equation for this reaction. If 6.5 g of zinc is used, calculate the volume of hydrogen gas produced at STP. (Atomic mass of Zn = 65 u, 1 mole of gas at STP = 22.4 L)