The following questions are pertaining to the laboratory preparation of Ammonia gas from Magnesium nitride:
(a) Write a balanced chemical equation for its preparation.
(b) Why is this method seldom used?
(c) How do you identify the gas formed?
(a) Mg3N2 + 6H2O → 3Mg(OH)2 + 2NH3
(b) Magnesium nitride is expensive, so this method is seldom used.
(c) Ammonia turns moist red litmus paper blue. It also forms dense white fumes of ammonium chloride when a glass rod dipped in concentrated hydrochloric acid is brought near the gas.
NH3 + HCl → NH4Cl
More ICSE Moderate level questions
Complete and balance the following equations: (a) NH4Cl + Ca(OH)2 → (b) CuSO4 + NH4OH → (c) Cu + Conc. HNO3 →
State one relevant observation for each of the following: (a) To the copper nitrate solution, initially few drops of sodium hydroxide solution is added and then added in excess. (b) Burning of ammonia in excess of oxygen. (c) Dry ammonia gas is passed over heated PbO.
State the terms/process for the following: (a) The energy released when an atom in the gaseous state accepts an electron to form an anion. (b) Tendency of an element to form chains of identical atoms. (c) The name of the process by which Ammonia is manufactured on a large scale. (d) A type of salt formed by partial replacement of hydroxyl radicals with an acid radical. (e) The ratio of the mass of a certain volume of gas to the same volume of hydrogen measured under the same conditions of temperature and pressure.
State a relevant reason for the following: [2] (a) Hydrogen chloride gas cannot be dried over quick lime. (b) Ammonia gas is not collected over water.
Mohan has three solutions P, Q and R having a pH of 13, 5 and 2 respectively. Which of the above solutions P, Q or R: (a) will react with Magnesium to liberate hydrogen gas? (b) will liberate ammonia gas when it reacts with ammonium chloride? (c) will contain molecules as well as ions?
Complete and balance the following equations: (a) C2H4Br2 + KOH (alcoholic) ⟶ (b) NH3 (excess) + Cl2 ⟶ (c)
Name the gas produced during each of the following reactions: (a) When copper is treated with hot, concentrated nitric acid. (b) When ammonia is burnt in an atmosphere of oxygen. (c) When ferrous sulphide reacts with dilute hydrochloric acid.
Given below is the industrial process for the manufacture of ammonia gas. Study the schematic diagram to answer the following questions. (a) Name the process. (b) Which catalyst is used in the above process? (c) In the above diagrammatic setup, how is ammonia gas separated from the unreacted gases to obtain liquid ammonia? (d) Which two properties of ammonia gas can be demonstrated by the Fountain Experiment?
Rewrite the following statements by adding the correct word as shown in the example: Example: Given Statement: Ammonia changes moist red litmus to blue. Correct Statement: Aqueous ammonia changes moist red litmus to blue. (a) Sulphuric acid acts as a dehydrating agent. (b) Ammonia reacts with chlorine to give ammonium chloride and nitrogen.
Match the Column A with Column B: Column A Column B (a) N2 + 3H2 ⇌ 2NH3 1. Vanadium Pentoxide (b) 4NH3 + 5O2 ⟶ 4NO + 6H2O 2. Nickel (c) 2SO2 + O2 ⇌ 2SO3 3. Iron (d) C2H4 + H2 ⟶ C2H6 4. Concentrated Sulphuric acid (e) CuSO4.5H2O ⟶ CuSO4 + 5H2O 5. Platinum
Ammonia gas is passed over heated copper (II) oxide in a combustion tube: (a) Name the gas evolved. (b) What will be the colour of the residue that is left in the combustion tube at the end of the reaction?
A student was instructed by the teacher to prepare and collect ammonia gas in the laboratory by using aluminium nitride. The student had set up the apparatus as shown in the diagram below. Study the given diagram and answer the following questions: (a) Name the substance X added through the thistle funnel by the student. (b) Write a balanced equation for the reaction occurring between Aluminium nitride and substance X. (c) Identify the substance Y. (d) State the function of Y. (e) Why could the student not collect ammonia gas at the end of the experiment?
