Question

match each chemical reaction with the type of reaction that best describes it. 2al + 6hcl → 2alcl₃ + 3h₂; ca + br₂ → cabr₂; 4nh₃ + 5o₂ → 4no + 6h₂o; 2nacl → 2na + cl₂; fes + 2hcl → fecl₂ + h₂s. synthesis; decomposition; single displacement; double displacement; combustion

Explanation:

To solve this, we analyze each reaction type:

1. Synthesis Reaction

A synthesis reaction combines two or more substances into one.

• Reaction: $\boldsymbol{\ce{Ca + Br2 -> CaBr2}}$ (Ca and $\ce{Br2}$ combine to form $\ce{CaBr2}$).

2. Decomposition Reaction

A decomposition reaction breaks one compound into simpler substances.

• Reaction: $\boldsymbol{\ce{2NaCl -> 2Na + Cl2}}$ (NaCl decomposes into Na and $\ce{Cl2}$).

3. Single Displacement Reaction

A single displacement reaction involves one element replacing another in a compound.

• Reaction: $\boldsymbol{\ce{2Al + 6HCl -> 2AlCl3 + 3H2}}$ (Al displaces H in HCl to form $\ce{AlCl3}$ and $\ce{H2}$).

4. Double Displacement Reaction

A double displacement reaction swaps ions between two compounds.

• Reaction: $\boldsymbol{\ce{FeS + 2HCl -> FeCl2 + H2S}}$ ($\ce{Fe^{2+}}$ and $\ce{H+}$ swap with $\ce{S^{2-}}$ and $\ce{Cl-}$).

5. Combustion Reaction

Combustion involves a substance reacting with $\ce{O2}$ (often producing oxides).

• Reaction: $\boldsymbol{\ce{4NH3 + 5O2 -> 4NO + 6H2O}}$ ($\ce{NH3}$ reacts with $\ce{O2}$ to form oxides of N and H₂O).

Final Matches:

• Synthesis: $\boldsymbol{\ce{Ca + Br2 -> CaBr2}}$
• Decomposition: $\boldsymbol{\ce{2NaCl -> 2Na + Cl2}}$
• Single Displacement: $\boldsymbol{\ce{2Al + 6HCl -> 2AlCl3 + 3H2}}$
• Double Displacement: $\boldsymbol{\ce{FeS + 2HCl -> FeCl2 + H2S}}$
• Combustion: $\boldsymbol{\ce{4NH3 + 5O2 -> 4NO + 6H2O}}$

Answer:

To solve this, we analyze each reaction type:

1. Synthesis Reaction

A synthesis reaction combines two or more substances into one.

• Reaction: $\boldsymbol{\ce{Ca + Br2 -> CaBr2}}$ (Ca and $\ce{Br2}$ combine to form $\ce{CaBr2}$).

2. Decomposition Reaction

A decomposition reaction breaks one compound into simpler substances.

• Reaction: $\boldsymbol{\ce{2NaCl -> 2Na + Cl2}}$ (NaCl decomposes into Na and $\ce{Cl2}$).

3. Single Displacement Reaction

A single displacement reaction involves one element replacing another in a compound.

• Reaction: $\boldsymbol{\ce{2Al + 6HCl -> 2AlCl3 + 3H2}}$ (Al displaces H in HCl to form $\ce{AlCl3}$ and $\ce{H2}$).

4. Double Displacement Reaction

A double displacement reaction swaps ions between two compounds.

• Reaction: $\boldsymbol{\ce{FeS + 2HCl -> FeCl2 + H2S}}$ ($\ce{Fe^{2+}}$ and $\ce{H+}$ swap with $\ce{S^{2-}}$ and $\ce{Cl-}$).

5. Combustion Reaction

Combustion involves a substance reacting with $\ce{O2}$ (often producing oxides).

• Reaction: $\boldsymbol{\ce{4NH3 + 5O2 -> 4NO + 6H2O}}$ ($\ce{NH3}$ reacts with $\ce{O2}$ to form oxides of N and H₂O).

Final Matches:

• Synthesis: $\boldsymbol{\ce{Ca + Br2 -> CaBr2}}$
• Decomposition: $\boldsymbol{\ce{2NaCl -> 2Na + Cl2}}$
• Single Displacement: $\boldsymbol{\ce{2Al + 6HCl -> 2AlCl3 + 3H2}}$
• Double Displacement: $\boldsymbol{\ce{FeS + 2HCl -> FeCl2 + H2S}}$
• Combustion: $\boldsymbol{\ce{4NH3 + 5O2 -> 4NO + 6H2O}}$