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Balance the following chemical equations by adding coefficients and classify each reaction by writing the correct abbreviation on the right-hand side.

Abbreviations:
- S: synthesis
- D: decomposition
- C: combustion
- SR: single replacement

11. [tex]\[\quad 2H_2 + \quad Cl_2 \rightarrow \quad 2HCl\][/tex]
- Reaction type: S (synthesis)

12. [tex]\[\quad C_2H_6 + \quad O_2 \rightarrow \quad CO_2 + \quad H_2O\][/tex]
- Reaction type: C (combustion)

13. [tex]\[\quad Al + \quad HCl \xrightarrow{O} \quad AlCl_3 + \quad H_2\][/tex]
- Reaction type: SR (single replacement)

14. [tex]\[\quad 2NaCl \rightarrow \quad 2Na + \quad Cl_2\][/tex]
- Reaction type: D (decomposition)

Answer :

Sure! Let's go through each chemical equation, balance them, and identify the type of reaction.

### Question 11:
Equation: [tex]\(2 \text{H}_2 + \text{Cl}_2 \rightarrow 2 \text{HCl}\)[/tex]

1. Balance the Equation:
- Start with the given equation: [tex]\( \text{H}_2 + \text{Cl}_2 \rightarrow \text{HCl} \)[/tex].
- To balance the hydrogen atoms, place a coefficient of 2 in front of [tex]\(\text{HCl}\)[/tex] to get [tex]\(2 \text{HCl}\)[/tex].
- Now we have: [tex]\(2 \text{H}_2 + \text{Cl}_2 \rightarrow 2 \text{HCl}\)[/tex].

2. Reaction Type:
- This is a synthesis reaction (S) because two or more reactants combine to form a single product.

### Question 12:
Equation: [tex]\(2 \text{C}_2\text{H}_6 + 7 \text{O}_2 \rightarrow 4 \text{CO}_2 + 6 \text{H}_2\text{O}\)[/tex]

1. Balance the Equation:
- Start with balancing the carbons: [tex]\(2 \text{C}_2\text{H}_6 \)[/tex] gives us [tex]\(4 \text{C}\)[/tex] in the reactants, so we need [tex]\(4 \text{CO}_2\)[/tex] in the products.
- Next, balance the hydrogens: [tex]\(2 \text{C}_2\text{H}_6 \)[/tex] gives us [tex]\(12 \text{H}\)[/tex] in the reactants, so we need [tex]\(6 \text{H}_2\text{O}\)[/tex] in the products.
- Finally, balance the oxygens. We have: [tex]\(4 \times 2 + 6\)[/tex] oxygens needed in products = 14 oxygens total, which requires [tex]\(7 \text{O}_2 \)[/tex] in the reactants.

2. Reaction Type:
- This is a combustion reaction (C), as it involves a hydrocarbon ([tex]\(\text{C}_2\text{H}_6\)[/tex]) reacting with oxygen ([tex]\(\text{O}_2\)[/tex]) to produce carbon dioxide ([tex]\(\text{CO}_2\)[/tex]) and water ([tex]\(\text{H}_2\text{O}\)[/tex]).

### Question 13:
Equation: [tex]\(2 \text{Al} + 6 \text{HCl} \rightarrow 2 \text{AlCl}_3 + 3 \text{H}_2\)[/tex]

1. Balance the Equation:
- Start with balancing the aluminum atoms. We place 2 before [tex]\(\text{AlCl}_3\)[/tex] because each [tex]\(\text{AlCl}_3\)[/tex] contains 1 aluminum atom, and we need to have two on each side.
- Next, hydrochloric acid [tex]\(\text{HCl}\)[/tex] should be 6 to provide 6 chloride ions for [tex]\(2 \text{AlCl}_3\)[/tex].
- Finally, balance hydrogen: 6 [tex]\(\text{H}\)[/tex] from [tex]\(6 \text{HCl}\)[/tex] will form [tex]\(3 \text{H}_2\)[/tex].

2. Reaction Type:
- This is a single replacement reaction (SR), where aluminum ([tex]\(\text{Al}\)[/tex]) replaces hydrogen in hydrochloric acid ([tex]\(\text{HCl}\)[/tex]) to form aluminum chloride ([tex]\(\text{AlCl}_3\)[/tex]) and hydrogen gas ([tex]\(\text{H}_2\)[/tex]).

### Question 14:
Equation: [tex]\(2 \text{NaCl} \rightarrow 2 \text{Na} + \text{Cl}_2\)[/tex]

1. Balance the Equation:
- Start with the provided equation [tex]\(\text{NaCl} \rightarrow \text{Na} + \text{Cl}_2\)[/tex].
- Two [tex]\(\text{Cl}\)[/tex] atoms are needed for [tex]\(\text{Cl}_2\)[/tex], so place a coefficient of 2 in front of [tex]\(\text{NaCl}\)[/tex] to balance both sodium and chlorine.

2. Reaction Type:
- This is a decomposition reaction (D), as a single compound [tex]\(\text{NaCl}\)[/tex] breaks down into two simpler substances [tex]\(\text{Na}\)[/tex] and [tex]\(\text{Cl}_2\)[/tex].

These are the balanced chemical equations and their respective reaction types.

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