Chemistry I Cp - Types Of Reactions

1. Calcium plus oxygen yields calcium oxide

Synthesis

Decomposition

Single replacement

Double replacement

The given chemical equation "calcium plus oxygen yields calcium oxide" represents a synthesis reaction. In synthesis reactions, two or more substances combine to form a single compound. In this case, calcium and oxygen combine to form calcium oxide. The reactants (calcium and oxygen) are combined to produce the product (calcium oxide), making it a synthesis reaction.

Explanation

The given chemical equation "calcium plus oxygen yields calcium oxide" represents a synthesis reaction. In synthesis reactions, two or more substances combine to form a single compound. In this case, calcium and oxygen combine to form calcium oxide. The reactants (calcium and oxygen) are combined to produce the product (calcium oxide), making it a synthesis reaction.

2. Potassium iodide combines with lead II nitrate to produce lead II iodide and potassium nitrate

Synthesis

Decomposition

Single replacement

Double replacement

In a double replacement reaction, the cations and anions of two different compounds switch places to form two new compounds. In this case, potassium iodide (KI) and lead II nitrate (Pb(NO3)2) react to form lead II iodide (PbI2) and potassium nitrate (KNO3). The potassium cation (K+) from potassium iodide combines with the nitrate anion (NO3-) from lead II nitrate to form potassium nitrate, while the lead II cation (Pb2+) from lead II nitrate combines with the iodide anion (I-) from potassium iodide to form lead II iodide. Hence, the reaction is a double replacement.

Explanation

In a double replacement reaction, the cations and anions of two different compounds switch places to form two new compounds. In this case, potassium iodide (KI) and lead II nitrate (Pb(NO3)2) react to form lead II iodide (PbI2) and potassium nitrate (KNO3). The potassium cation (K+) from potassium iodide combines with the nitrate anion (NO3-) from lead II nitrate to form potassium nitrate, while the lead II cation (Pb2+) from lead II nitrate combines with the iodide anion (I-) from potassium iodide to form lead II iodide. Hence, the reaction is a double replacement.

3. Magnesium plus hydrochloric acid produces magnesium chloride and hydrogen

Synthesis

Decomposition

Single replacement

Double replacement

In a single replacement reaction, one element replaces another element in a compound. In this case, magnesium (Mg) replaces hydrogen (H) in hydrochloric acid (HCl) to form magnesium chloride (MgCl2) and hydrogen gas (H2). This reaction can be represented by the equation: Mg + 2HCl -> MgCl2 + H2.

Explanation

In a single replacement reaction, one element replaces another element in a compound. In this case, magnesium (Mg) replaces hydrogen (H) in hydrochloric acid (HCl) to form magnesium chloride (MgCl2) and hydrogen gas (H2). This reaction can be represented by the equation: Mg + 2HCl -> MgCl2 + H2.

4. Sodium bromide reacts with fluorine to produce sodium fluoride and bromine gas

Synthesis

Decomposition

Single replacement

Double replacement

In a single replacement reaction, one element replaces another element in a compound. In this case, sodium bromide (NaBr) reacts with fluorine (F2) to produce sodium fluoride (NaF) and bromine gas (Br2). The sodium atom in sodium bromide is replaced by the fluorine atom, resulting in the formation of sodium fluoride, while the bromine atom is released as bromine gas. Therefore, the given reaction is an example of a single replacement reaction.

Explanation

In a single replacement reaction, one element replaces another element in a compound. In this case, sodium bromide (NaBr) reacts with fluorine (F2) to produce sodium fluoride (NaF) and bromine gas (Br2). The sodium atom in sodium bromide is replaced by the fluorine atom, resulting in the formation of sodium fluoride, while the bromine atom is released as bromine gas. Therefore, the given reaction is an example of a single replacement reaction.

5. Barium hydroxide combines with aluminum sulfate to produce aluminum hydroxude and barium sulfate

Synthesis

Decomposition

Single replacement

Double replacement

In a double replacement reaction, the cations and anions of two different compounds switch places to form two new compounds. In this case, barium hydroxide (Ba(OH)2) combines with aluminum sulfate (Al2(SO4)3) to produce aluminum hydroxide (Al(OH)3) and barium sulfate (BaSO4). The cations (Ba and Al) switch places, as well as the anions (OH and SO4), resulting in the formation of two new compounds. Therefore, the given reaction is an example of a double replacement reaction.

Explanation

In a double replacement reaction, the cations and anions of two different compounds switch places to form two new compounds. In this case, barium hydroxide (Ba(OH)2) combines with aluminum sulfate (Al2(SO4)3) to produce aluminum hydroxide (Al(OH)3) and barium sulfate (BaSO4). The cations (Ba and Al) switch places, as well as the anions (OH and SO4), resulting in the formation of two new compounds. Therefore, the given reaction is an example of a double replacement reaction.