Classify each of the following reactions as asynthesis, decomposition, single-displacement, double-displacement, or combustion reaction: a. N2(g) + 3H2(g)→ 2NH3(g) b. 2Li(s) + 2H2O(l) → 2LiOH(aq) + H2(g) c. 2NaNO3(s) → 2NaNO2(s) + O 2(g) d. 2C6H14(l) + 19O2(g) → 12CO2(g) + 14H2O(l)

a. N2(g) + 3H2(g)→ 2NH3(g) ===> synthesis

b. 2Li(s) + 2H2O(l) → 2LiOH(aq) + H2(g) ===> single-displacement

c. 2NaNO3(s) → 2NaNO2(s) + O2(g)  ===> decomposition

d. 2C6H14(l) + 19O2(g) → 12CO2(g) + 14H2O(l) ===> combustion

Explanation:

A synthesis reaction occurs when two or more reactants combine to form a single product. This type of reaction is represented by the general equation: A + B → AB. An example of a synthesis reaction is the combination of sodium (Na) and chlorine (Cl) to produce sodium chloride (NaCl). N2(g) + 3H2(g)→ 2NH3(g) is a good example. Single Replacement Reactions. A single replacement reaction occurs when one element replaces another in a single compound. An example of a single replacement reaction occurs when potassium (K) reacts with water (H2O). A colorless solid compound named potassium hydroxide (KOH) forms, and hydrogen gas (H2) is liberated. another example is  2Li(s) + 2H2O(l) → 2LiOH(aq) + H2(g).A decomposition reaction occurs when one reactant breaks down into two or more products. This can be represented by the general equation: AB → A + B. Examples of decomposition reactions include the breakdown of hydrogen peroxide to water and oxygen, and the breakdown of water to hydrogen and oxygen. Another example is 2NaNO3(s) → 2NaNO2(s) + O2(g)Combustion reactions always involve molecular oxygen O2. Anytime anything burns, it reacts with oxygen. Combustion reactions are almost always exothermic (i.e., they give off heat). When organic molecules combust the reaction products are carbon dioxide and water. Example 2C6H14(l) + 19O2(g) → 12CO2(g) + 14H2O(l)

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