Predicting Products of Chemical Reactions Quiz

Hydrogen gas reacts with oxygen gas in a synthesis (combustion) reaction to produce water. The balanced reaction is 2H2 + O2 → 2H2O, making water the correct product.

The reaction between sodium bicarbonate and an acid is an acid-base neutralization reaction that also produces carbon dioxide gas. This gas evolution is characteristic of such reactions.

When calcium carbonate (CaCO3) is heated, it decomposes into calcium oxide (CaO) and carbon dioxide (CO2). This is a common example of a thermal decomposition reaction in chemistry.

Sodium reacts with chlorine in a synthesis reaction to form sodium chloride, which is correctly balanced as 2Na + Cl2 → 2NaCl. This is a fundamental reaction in inorganic chemistry.

When magnesium burns in oxygen, it reacts to form magnesium oxide (MgO), a typical synthesis reaction involving a metal and oxygen. This reaction is highly exothermic and commonly observed in demonstrations.

A double displacement reaction occurs between lead(II) nitrate and potassium iodide, resulting in the formation of insoluble lead(II) iodide as a precipitate along with potassium nitrate in solution. This is a classic example of a precipitation reaction.

When silver nitrate reacts with sodium chloride, a precipitation reaction occurs where insoluble silver chloride forms. The remaining ions form sodium nitrate, making it a typical double displacement reaction.

The combustion of propane in excess oxygen produces carbon dioxide and water. The balanced equation is C3H8 + 5O2 → 3CO2 + 4H2O, which confirms the stoichiometry of the reactants and products.

Zinc is more reactive than copper, so it displaces copper from copper(II) sulfate in a single replacement reaction, forming zinc sulfate and depositing copper metal. This is a classic displacement reaction demonstrating the activity series of metals.

Copper(II) ions react with ammonia to form a deep blue tetraamminecopper(II) complex. This complex formation is a characteristic reaction in qualitative analysis for copper.

The reaction between iron(III) ions and thiocyanate ions produces a blood-red iron(III) thiocyanate complex. This reaction is commonly used as a confirmatory test for Fe3+ in solution.

Aluminum is normally protected by an oxide layer that prevents it from reacting with water. When the metal is powdered or the oxide layer is removed, aluminum can react with water to produce aluminum hydroxide and hydrogen gas.

Barium sulfate is highly insoluble in water and precipitates out when barium chloride reacts with sulfuric acid. This is a standard precipitation reaction based on established solubility rules.

The formation of an ester from acetic acid and ethanol is a condensation reaction, specifically an esterification, where water is removed as a byproduct. This reaction mechanism is characteristic of combining a carboxylic acid with an alcohol.

In an acidic medium, hydrogen peroxide reduces the purple permanganate ion to nearly colorless manganese(II) ions. This redox reaction is a textbook example of permanganate reduction.

The reaction between sodium phosphate and calcium chloride is a double displacement reaction that produces an insoluble calcium phosphate precipitate and soluble sodium chloride. The reaction follows the solubility rules governing phosphate salts.

A metal oxide is basic in nature and reacts with an acid like hydrochloric acid to form a salt (metal chloride) and water. This acid-base reaction is predictable and fundamental in inorganic chemistry.

In acidic conditions, lead(IV) oxide oxidizes iodide ions to iodine while being reduced to lead(II), which then precipitates as lead(II) iodide. This complex redox reaction demonstrates both oxidation and reduction processes simultaneously.

NO reacts with O2 in the atmosphere to form nitrogen dioxide (NO2), a brown gas that contributes to photochemical smog. The reaction is represented by 2NO + O2 → 2NO2, indicating a clear and direct product prediction.

Alkali metals react exothermically with water to produce metal hydroxides and hydrogen gas. This reaction is well-known for its vigorous nature and is a classic demonstration of the properties of alkali metals.