Ammonia Preparation and Reactions Quiz

Heating ammonium salts (like NH₄Cl or (NH₄)₂SO₄) with substances like quicklime (CaO) or slaked lime (Ca(OH)₂), or caustic soda (NaOH), to produce ammonia gas.

An ionic compound with the chemical formula NH₄Cl, used in the lab to prepare ammonia.

A chemical compound with the formula CaO, used to produce ammonia and dry the gas.

A colorless gas with a pungent odor, produced by heating ammonium salts with a base.

Removing water vapor from ammonia gas using calcium oxide (CaO), forming calcium hydroxide.

A method for collecting a gas lighter than air, like ammonia.

The ratio of the masses of reactants in a chemical reaction.

The ratio of ammonium chloride to calcium oxide for the laboratory preparation of ammonia.

Ammonia is a gas at room temperature.

Ammonia is colourless.

Ammonia has a pungent smell.

Ammonia taste is slightly basic.

Ammonia liquefies at -33.41°C at normal pressure.

A concentrated aqueous solution of ammonia (30%).

Ammonia has a high vapor pressure at ambient temperatures.

Ammonia is lighter than air (vapor density ~8.5).

Ammonia is highly soluble in water.

Ammonia acts as a weak base in water.

Ammonia gas reacts with HCl gas to form ammonium chloride solid.

Ammonia reacts with concentrated sulfuric acid to form ammonium sulfate.

Ammonia reacts with nitric acid to form ammonium nitrate.

Ammonia can reduce metal oxides at high temperatures.

A method to industrially produce ammonia by reacting nitrogen and hydrogen under high pressure and temperature.

Ammonia is used to make fertilizers, nitric acid, and some medicines.

Urea is produced from ammonia and carbon dioxide in industrial settings.

Urea is a key component in fertilizers, plastics and some important medicines

An industrial process that produces ammonia. It is also called Haber's process.

The chemical formula for hydrogen sulfide is H₂S.

The vapor density of hydrogen sulfide is 17.

Not applicable, as the content only focuses on its laboratory preparation, not industrial uses.

Laboratory preparation of hydrogen sulfide involves reacting ferrous sulfide with dilute sulfuric acid.

Aqueous ammonia reacts with metal salts to form precipitates of metal hydroxides, whose colors can identify the metal.

Ammonia reacts with copper sulfate solutions to first form a pale blue precipitate of copper hydroxide, which then dissolves in excess ammonia to form a deep blue solution of cupric ammonium sulfate.

A reagent for detecting ammonia; a potassium mercuric iodide solution that reacts with ammonia to produce a brown precipitate.

Hot sodium reacts with dry ammonia gas to form sodamide and hydrogen gas.

Demonstrates the high solubility of ammonia in water using a flask filled with ammonia gas. Water from a dropper draws the litmus solution into the flask.

Phenolphthalein turns an ammonia solution pink. The color disappears when the ammonia evaporates.

The precipitate formed when iron(II) sulfate reacts with ammonium hydroxide is dirty green.

Reaction of iron(III) chloride with ammonium hydroxide yields a reddish-brown precipitate of iron(III) hydroxide.

Chromium(III) salts forms a green precipitate when reacted with ammonium hydroxide.

Aluminum salts forms a white and gelatinous precipitate when reacted with ammonium hydroxide.

A bent glass tube with a Wolff bottle and ferrous sulfide, submerged in water, to produce H₂S.

Collecting heavier-than-air gas by upward displacement in a gas jar.

Hydrogen gas, sulfuric acid vapor, and water vapor contained in the produced H₂S gas.

Removing impurities like H₂SO₄ vapor with NaHS solution, and water vapor using P₂O₅.

A special apparatus for producing H₂S gas, using FeS and diluted H₂SO₄.

In the Kipp's apparatus, a stopper regulates gas pressure, allowing controlled release, then re-starting the reaction.

Concentrated sulfuric acid isn't suitable to produce H₂S as it oxidizes H₂S into sulfur and sulfur dioxide.

Passing hydrogen sulfide gas through a freshly prepared sodium nitroprusside solution forms a violet complex, identifying the gas.

Prepare H₂S in a fume hood, slowly, and seal the collection container immediately to prevent escape.

H₂S in the air reacts with silver, turning it black, and with lead in paint, also making it black via PbS.

Heating a mixture of ammonium chloride and sodium nitrite produces nitrogen gas.

Nitrogen is used in ammonia production, fertilizer making, inert atmospheres, gas thermometers, and as a coolant (liquid nitrogen).

The chemical formula for nitrogen gas is N₂.

H₂S is a poisonous gas at room temperature.

Concentrations above 5 ppm can cause fainting in humans.

H₂S is soluble in cold water, forming an acidic solution.

H₂S smells like rotten eggs.

High pressure liquefies H₂S into a colorless liquid.

H₂S is denser than air (vapour density = 17.6).

H₂S burns in oxygen, producing sulfur dioxide and steam.

H₂S reduces potassium dichromate, changing its color.

H₂S reacts with metal salt solutions to form metal sulphides.

The copper sulfide produced in a reaction with H₂S is black.

The lead sulfide produced in a reaction with H₂S is black.

The silver sulfide produced in a reaction with H₂S is black.

The industrial method for producing sulfuric acid ($H₂SO₄$).

Conversion of sulfur dioxide ($SO₂$) to sulfur trioxide ($SO₃$) using a catalyst.

A substance that speeds up the $SO₂$ oxidation reaction without being consumed.

An intermediate product formed by absorbing $SO₃$ in concentrated $H₂SO₄$.

Substances that can negatively impact the catalyst and reaction efficiency.

The crucial step of absorbing $SO₃$ into concentrated $H₂SO₄$ to form oleum and then sulfuric acid

Purification of sulfur, oxidation of $SO_2$ to $SO_3$, absorption of $SO_3$ in concentrated $H₂SO₄$, Production of concentrated $H₂SO₄$.

Nitrogen exists as a gas at standard temperature and pressure (STP).

Nitrogen is relatively unreactive at lower temperatures due to its strong triple bond. However, it reacts at high temperatures.

Converting atmospheric nitrogen into usable nitrogen compounds, often for fertilizers.

Lightning converting nitrogen & oxygen into compounds like nitric acid.

Industrial processes used to create nitrogen compounds for fertilizers.

Nitrogen reacts with hydrogen at high pressure and temperature to produce ammonia.

Nitrogen reacts with oxygen in high temperature to form Nitric Oxide.

Nitrogen reacts with heated magnesium to form magnesium nitride.

Nitrogen reacts with heated calcium carbide to produce calcium cyanamide.

Hydrogen and chlorine react to form hydrochloric acid.

Industrial process to create Nitric acid using oxidation methods or other reactions.

Industry process to produce sulphuric acid using various methods.

Chlorine gas reacts with hydrogen gas to produce hydrochloric acid.

Hydrochloric acid is made by reacting chlorine and hydrogen gas.

A method to produce hydrochloric acid from table salt and sulfuric acid.

A process for manufacturing nitric acid from ammonia.

Ammonia and air react over a catalyst to form nitric oxide.

Nitric oxide reacts with oxygen to form nitrogen dioxide.

Nitrogen dioxide reacts with water to form nitric acid.

A process for manufacturing sulfuric acid.

Burning sulfur or iron pyrites to make sulfur dioxide.

Sulfur dioxide is oxidized to sulfur trioxide using a catalyst.

Sulfur trioxide reacts with sulfuric acid to form oleum.