Nitrogen and Its Compounds
Chemistry ⇒ Chemistry of Non-metals and Their Compounds
Nitrogen and Its Compounds starts at 9 and continues till grade 12.
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Compare and contrast the structures and uses of nitric acid (HNO3) and nitrous acid (HNO2).
Describe the Ostwald process for the industrial manufacture of nitric acid.
Describe the role of nitrogen in the atmosphere and explain why it is considered an essential element for living organisms.
Discuss the environmental impact of excessive use of nitrogen-based fertilizers.
Explain the process of nitrogen fixation and its importance in the nitrogen cycle.
Explain the steps involved in the laboratory preparation of ammonia gas.
Write a short note on the physical and chemical properties of ammonia (NH3).
A sample of nitrogen dioxide (NO2) weighing 92 g is dissolved in water to produce nitric acid and nitric oxide according to the following reaction: 3NO2 + H2O → 2HNO3 + NO. Calculate the mass of nitric acid formed. (Atomic masses: N = 14, O = 16, H = 1)
Ammonia (NH3) is prepared in the laboratory by heating ammonium chloride (NH4Cl) with slaked lime (Ca(OH)2). Write the balanced chemical equation for this reaction. If 10 g of NH4Cl is used, calculate the mass of ammonia gas produced, assuming 100% yield. (Atomic masses: N = 14, H = 1, Cl = 35.5, Ca = 40, O = 16)
Describe the chemical test used to distinguish between ammonia gas and nitrogen gas. Explain the observations and write the relevant chemical equations.
Explain the steps involved in the industrial preparation of nitric acid by the Ostwald process. Write all the relevant chemical equations and calculate the total number of moles of NO2 formed when 2 moles of ammonia are used, assuming complete conversion.
Explain why nitrogen is relatively unreactive at room temperature, but forms a variety of compounds at higher temperatures or in the presence of catalysts. Relate your answer to the molecular structure and bonding in nitrogen.
