Predicting Products of Chemical Reactions | PDF | Ion | Chemical ... - Free Printable

Problem Overview:

The task involves predicting the products of various chemical reactions and identifying the type of reaction (synthesis, decomposition, single replacement, double replacement, or combustion). The goal is to balance the equations and determine the correct products based on the reactants provided.

Solution Approach:

1. Identify the Type of Reaction: Determine whether the reaction is synthesis, decomposition, single replacement, double replacement, or combustion.
2. Predict Products:
- Synthesis: Two or more substances combine to form one product.
- Decomposition: One substance breaks down into two or more simpler substances.
- Single Replacement: One element replaces another in a compound.
- Double Replacement: Ions from two compounds switch places to form two new compounds.
- Combustion: A substance reacts with oxygen to produce carbon dioxide and water (for hydrocarbons).
3. Balance the Equation: Ensure that the number of atoms of each element is the same on both sides of the equation.

Detailed Solutions:

#### Combustion Reactions:
1. C₆H₁₂ + O₂ →
- Combustion of a hydrocarbon produces CO₂ and H₂O.
- Balanced Equation:
\[
\text{C}_6\text{H}_{12} + 9\text{O}_2 \rightarrow 6\text{CO}_2 + 6\text{H}_2\text{O}
\]

2. C₄H₆ + O₂ →
- Combustion of a hydrocarbon produces CO₂ and H₂O.
- Balanced Equation:
\[
2\text{C}_4\text{H}_6 + 13\text{O}_2 \rightarrow 8\text{CO}_2 + 6\text{H}_2\text{O}
\]

3. C₅H₁₀O₃ + O₂ →
- Combustion of an organic compound produces CO₂ and H₂O. The oxygen in the compound also contributes to the overall oxygen balance.
- Balanced Equation:
\[
\text{C}_5\text{H}_{10}\text{O}_3 + 5\text{O}_2 \rightarrow 5\text{CO}_2 + 5\text{H}_2\text{O}
\]

#### Synthesis Reaction:
4. Mg + I₂ →
- Synthesis: Mg combines with I₂ to form MgI₂.
- Balanced Equation:
\[
\text{Mg} + \text{I}_2 \rightarrow \text{MgI}_2
\]

#### Double Displacement Reactions:
5. CuCl₂ + H₂S →
- Double displacement: Cu²⁺ and S²⁻ form CuS (insoluble), and H⁺ and Cl⁻ form HCl.
- Balanced Equation:
\[
\text{CuCl}_2 + \text{H}_2\text{S} \rightarrow \text{CuS} \downarrow + 2\text{HCl}
\]

6. NaOH + HClO₄ →
- Double displacement: Na⁺ and ClO₄⁻ form NaClO₄, and OH⁻ and H⁺ form H₂O.
- Balanced Equation:
\[
\text{NaOH} + \text{HClO}_4 \rightarrow \text{NaClO}_4 + \text{H}_2\text{O}
\]

#### Decomposition Reaction:
7. ZnCO₃ + heat →
- Decomposition: ZnCO₃ breaks down into ZnO and CO₂.
- Balanced Equation:
\[
\text{ZnCO}_3 \xrightarrow{\text{heat}} \text{ZnO} + \text{CO}_2 \uparrow
\]

#### Single Replacement Reaction:
8. HCl + Zn →
- Single replacement: Zn displaces H⁺ to form ZnCl₂ and H₂ gas.
- Balanced Equation:
\[
\text{Zn} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \uparrow
\]

#### Other Reactions:
9. Na + MgCl₂ →
- Single replacement: Na displaces Mg to form NaCl and Mg.
- Balanced Equation:
\[
2\text{Na} + \text{MgCl}_2 \rightarrow 2\text{NaCl} + \text{Mg}
\]

10. CaCl₂ + K₂CO₃ →
- Double displacement: Ca²⁺ and CO₃²⁻ form CaCO₃ (insoluble), and K⁺ and Cl⁻ form KCl.
- Balanced Equation:
\[
\text{CaCl}_2 + \text{K}_2\text{CO}_3 \rightarrow \text{CaCO}_3 \downarrow + 2\text{KCl}
\]

11. K + Cl₂ →
- Synthesis: K reacts with Cl₂ to form KCl.
- Balanced Equation:
\[
2\text{K} + \text{Cl}_2 \rightarrow 2\text{KCl}
\]

12. BaCl₂ + K₃PO₄ →
- Double displacement: Ba²⁺ and PO₄³⁻ form Ba₃(PO₄)₂ (insoluble), and K⁺ and Cl⁻ form KCl.
- Balanced Equation:
\[
3\text{BaCl}_2 + 2\text{K}_3\text{PO}_4 \rightarrow \text{Ba}_3(\text{PO}_4)_2 \downarrow + 6\text{KCl}
\]

13. H₂SO₄ + KOH →
- Double displacement: H⁺ and OH⁻ form H₂O, and K⁺ and SO₄²⁻ form K₂SO₄.
- Balanced Equation:
\[
\text{H}_2\text{SO}_4 + 2\text{KOH} \rightarrow \text{K}_2\text{SO}_4 + 2\text{H}_2\text{O}
\]

14. Al₂(CO₃)₃ + heat →
- Decomposition: Al₂(CO₃)₃ breaks down into Al₂O₃ and CO₂.
- Balanced Equation:
\[
\text{Al}_2(\text{CO}_3)_3 \xrightarrow{\text{heat}} \text{Al}_2\text{O}_3 + 3\text{CO}_2 \uparrow
\]

15. Al + O₂ →
- Synthesis: Al reacts with O₂ to form Al₂O₃.
- Balanced Equation:
\[
4\text{Al} + 3\text{O}_2 \rightarrow 2\text{Al}_2\text{O}_3
\]

16. Pb(NO₃)₂ + KOH →
- Double displacement: Pb²⁺ and OH⁻ form Pb(OH)₂ (insoluble), and K⁺ and NO₃⁻ form KNO₃.
- Balanced Equation:
\[
\text{Pb(NO}_3)_2 + 2\text{KOH} \rightarrow \text{Pb(OH)}_2 \downarrow + 2\text{KNO}_3
\]

17. H₂SO₄ + BaCl₂ →
- Double displacement: Ba²⁺ and SO₄²⁻ form BaSO₄ (insoluble), and H⁺ and Cl⁻ form HCl.
- Balanced Equation:
\[
\text{H}_2\text{SO}_4 + \text{BaCl}_2 \rightarrow \text{BaSO}_4 \downarrow + 2\text{HCl}
\]

18. Ca + AgCl →
- Single replacement: Ca does not displace Ag because Ca is less reactive than Ag. No reaction occurs.
- Balanced Equation:
\[
\text{No reaction}
\]

19. H₃PO₄ + FeBr₃ →
- Double displacement: H₃PO₄ and FeBr₃ do not form insoluble precipitates or gases, so no reaction occurs.
- Balanced Equation:
\[
\text{No reaction}
\]

20. Li + N₂ →
- Synthesis: Li reacts with N₂ to form Li₃N.
- Balanced Equation:
\[
6\text{Li} + \text{N}_2 \rightarrow 2\text{Li}_3\text{N}
\]

21. HCl + Mg(OH)₂ →
- Double displacement: H⁺ and OH⁻ form H₂O, and Mg²⁺ and Cl⁻ form MgCl₂.
- Balanced Equation:
\[
2\text{HCl} + \text{Mg(OH)}_2 \rightarrow \text{MgCl}_2 + 2\text{H}_2\text{O}
\]

22. Mg(OH)₂ + heat →
- Decomposition: Mg(OH)₂ breaks down into MgO and H₂O.
- Balanced Equation:
\[
\text{Mg(OH)}_2 \xrightarrow{\text{heat}} \text{MgO} + \text{H}_2\text{O}
\]

23. Fe(OH)₃ + heat →
- Decomposition: Fe(OH)₃ breaks down into Fe₂O₃ and H₂O.
- Balanced Equation:
\[
2\text{Fe(OH)}_3 \xrightarrow{\text{heat}} \text{Fe}_2\text{O}_3 + 3\text{H}_2\text{O}
\]

Final Answer:

\[
\boxed{
\begin{array}{ll}
\text{1. } & \text{C}_6\text{H}_{12} + 9\text{O}_2 \rightarrow 6\text{CO}_2 + 6\text{H}_2\text{O} \\
\text{2. } & 2\text{C}_4\text{H}_6 + 13\text{O}_2 \rightarrow 8\text{CO}_2 + 6\text{H}_2\text{O} \\
\text{3. } & \text{C}_5\text{H}_{10}\text{O}_3 + 5\text{O}_2 \rightarrow 5\text{CO}_2 + 5\text{H}_2\text{O} \\
\text{4. } & \text{Mg} + \text{I}_2 \rightarrow \text{MgI}_2 \\
\text{5. } & \text{CuCl}_2 + \text{H}_2\text{S} \rightarrow \text{CuS} \downarrow + 2\text{HCl} \\
\text{6. } & \text{NaOH} + \text{HClO}_4 \rightarrow \text{NaClO}_4 + \text{H}_2\text{O} \\
\text{7. } & \text{ZnCO}_3 \xrightarrow{\text{heat}} \text{ZnO} + \text{CO}_2 \uparrow \\
\text{8. } & \text{Zn} + 2\text{HCl} \rightarrow \text{ZnCl}_2 + \text{H}_2 \uparrow \\
\text{9. } & 2\text{Na} + \text{MgCl}_2 \rightarrow 2\text{NaCl} + \text{Mg} \\
\text{10. } & \text{CaCl}_2 + \text{K}_2\text{CO}_3 \rightarrow \text{CaCO}_3 \downarrow + 2\text{KCl} \\
\text{11. } & 2\text{K} + \text{Cl}_2 \rightarrow 2\text{KCl} \\
\text{12. } & 3\text{BaCl}_2 + 2\text{K}_3\text{PO}_4 \rightarrow \text{Ba}_3(\text{PO}_4)_2 \downarrow + 6\text{KCl} \\
\text{13. } & \text{H}_2\text{SO}_4 + 2\text{KOH} \rightarrow \text{K}_2\text{SO}_4 + 2\text{H}_2\text{O} \\
\text{14. } & \text{Al}_2(\text{CO}_3)_3 \xrightarrow{\text{heat}} \text{Al}_2\text{O}_3 + 3\text{CO}_2 \uparrow \\
\text{15. } & 4\text{Al} + 3\text{O}_2 \rightarrow 2\text{Al}_2\text{O}_3 \\
\text{16. } & \text{Pb(NO}_3)_2 + 2\text{KOH} \rightarrow \text{Pb(OH)}_2 \downarrow + 2\text{KNO}_3 \\
\text{17. } & \text{H}_2\text{SO}_4 + \text{BaCl}_2 \rightarrow \text{BaSO}_4 \downarrow + 2\text{HCl} \\
\text{18. } & \text{No reaction} \\
\text{19. } & \text{No reaction} \\
\text{20. } & 6\text{Li} + \text{N}_2 \rightarrow 2\text{Li}_3\text{N} \\
\text{21. } & 2\text{HCl} + \text{Mg(OH)}_2 \rightarrow \text{MgCl}_2 + 2\text{H}_2\text{O} \\
\text{22. } & \text{Mg(OH)}_2 \xrightarrow{\text{heat}} \text{MgO} + \text{H}_2\text{O} \\
\text{23. } & 2\text{Fe(OH)}_3 \xrightarrow{\text{heat}} \text{Fe}_2\text{O}_3 + 3\text{H}_2\text{O} \\
\end{array}
}
\]