This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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a) i) The gas being produced is dinitrogen monoxide (or nitrous oxide). ii) The equation for the thermal decomposition of ammonium nitrate is: NH_4NO_3(s) N_2O(g) + 2H_2O(g) iii) The gas is collected over hot water because dinitrogen monoxide is sparingly soluble in water, and its solubility decreases further in hot water. This method ensures maximum collection of the gas. iv) When burning sulphur is lowered into a gas jar containing dinitrogen monoxide: • Observation: The sulphur burns with a brighter blue flame. • Explanation: Dinitrogen monoxide decomposes upon heating to produce nitrogen and oxygen (2N_2O(g) 2N_2(g) + O_2(g)). The oxygen produced supports the combustion of sulphur, causing it to burn more vigorously. b) i) The catalyst used during catalytic oxidation of ammonia is platinum (or platinum-rhodium alloy). ii) Nitrogen (IV) oxide (NO_2) is formed from nitrogen monoxide (NO) and oxygen. The chemical equation for its formation is: 2NO(g) + O_2(g) 2NO_2(g) iii) Two physical differences between Nitrogen (I) oxide (N_2O) and Nitrogen (IV) oxide (NO_2) are: • Color: N_2O is a colorless gas, while NO_2 is a reddish-brown gas. • Odor: N_2O has a sweet smell, while NO_2 has a pungent, suffocating smell. c) i) The apparatus must be made of glass because concentrated nitric acid is highly corrosive and reacts with many materials, especially metals. Glass is inert to concentrated nitric acid, preventing unwanted reactions and contamination. ii) (I) To identify the species oxidized, we determine the change in oxidation states: • In S_(s), the oxidation state of S is 0. • In H_2SO_4(aq), the oxidation state of S is +6. • In HNO_3(aq), the oxidation state of N is +5. • In NO_2(g), the oxidation state of N is +4. The oxidation state of sulphur increases from 0 to +6, indicating oxidation. The species oxidized is sulphur (S). (II) Pure nitric acid is colorless, but the product during its preparation is usually pale yellow because nitric acid decomposes when exposed to light or heat, forming nitrogen dioxide (NO_2). Nitrogen dioxide is a reddish-brown gas that dissolves in the nitric acid, imparting a pale yellow color. The decomposition reaction is: 4HNO_3(aq) 4NO_2(g) + O_2(g) + 2H_2O(l) Send me the next one 📸