Types of Chemical Reactions: Videos & Practice Problems

Chemical reactions involve the transformation of reactants into products, categorized into types such as redox, combination, decomposition, combustion, single displacement, and double displacement. In combination reactions, multiple reactants yield one product, while decomposition reactions split one reactant into several products. Combustion typically involves carbon-containing compounds reacting with oxygen to produce water and carbon dioxide. Displacement reactions involve elements swapping places in compounds, crucial for understanding ionic compounds and reaction mechanisms. Recognizing these types enhances comprehension of complex chemical equations and processes.

Types of Chemical Reactions Concept 1

Chemical reactions are fundamental processes where reactants undergo transformation to form new products. The classification of these reactions is primarily based on the changes that reactants experience and the nature of the products formed. One significant category of chemical reactions is redox reactions, characterized by the transfer of electrons between reactants.

Among the various types of chemical reactions, combination reactions involve multiple reactants merging to create a single product. For example, when solid sodium (Na) reacts with aqueous hypochlorite (ClO), they combine to form sodium hypochlorite (NaClO).

In contrast, decomposition reactions represent the reverse process, where a single reactant breaks down into multiple products. A classic example is the electrolysis of water (H₂O), which can be separated into hydrogen gas (H₂) and oxygen gas (O₂) when sufficient energy is applied.

Combustion reactions typically involve organic compounds containing carbon and hydrogen, or carbon, hydrogen, and oxygen. These compounds react with oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O). Recognizing the characteristics of combustion reactions is essential, even if balancing the equations is not the primary focus at this stage.

Single displacement reactions occur when a single element replaces another element in a compound. For instance, when zinc (Zn) reacts with copper(II) sulfate (CuSO₄), zinc displaces copper, resulting in zinc sulfate (ZnSO₄) and free copper (Cu).

Lastly, double displacement reactions involve the exchange of ions between two reacting compounds. An example is the reaction between barium nitrate (Ba(NO₃)₂) and sodium sulfate (Na₂SO₄), where barium (Ba) swaps places with sodium (Na), leading to the formation of barium sulfate (BaSO₄) and sodium nitrate (NaNO₃).

Understanding these different types of chemical reactions and their defining features is crucial, as it lays the groundwork for tackling more complex chemical equations and reactions in future studies.

Types of Chemical Reactions Example 1

To balance the chemical equation for the decomposition of ammonium nitrate, which breaks down into dinitrogen monoxide and water, we start by identifying the reactants and products involved. The unbalanced equation can be represented as:

NH₄NO₃ → N₂O + H₂O

Initially, we have:

• 2 nitrogen (N) atoms
• 4 hydrogen (H) atoms
• 3 oxygen (O) atoms

On the product side, we have:

• 2 nitrogen (N) atoms
• 2 hydrogen (H) atoms
• 2 oxygen (O) atoms

To balance the equation, we notice that the nitrogen atoms are already equal. However, the hydrogen and oxygen atoms are not balanced. To address this, we can place a coefficient of 2 in front of water (H₂O) on the product side:

NH₄NO₃ → N₂O + 2 H₂O

Now, the product side has:

• 2 nitrogen (N) atoms
• 4 hydrogen (H) atoms (from 2 H₂O)
• 3 oxygen (O) atoms (1 from N₂O and 2 from 2 H₂O)

Thus, the balanced equation is:

NH₄NO₃ → N₂O + 2 H₂O

This reaction is classified as a decomposition reaction, where a single reactant (ammonium nitrate) breaks down into multiple products (dinitrogen monoxide and water).

Ibuprofen is used as an anti-inflammatory agent used to deal with pain and bring down fevers. If it has a molecular formula of C₁₃H₁₈O₂, determine the balanced combustion reaction when it is subjected to high temperatures.

Ibuprofen, with the molecular formula C₁₃H₁₈O₂, serves as an anti-inflammatory agent effective in alleviating pain and reducing fevers. When subjected to high temperatures, it undergoes a combustion reaction, where it reacts with oxygen to produce carbon dioxide (CO₂) and water (H₂O) as byproducts.

To derive the balanced combustion reaction, we start by identifying the number of each type of atom in the reactants and products. The initial counts for ibuprofen are 13 carbons, 18 hydrogens, and 2 oxygens. The combustion reaction can be represented as:

C₁₃H₁₈O₂ + O₂ → H₂O + CO₂

To balance the equation, we first adjust the coefficients for carbon and hydrogen. Placing a coefficient of 13 in front of CO₂ accounts for the 13 carbon atoms:

C₁₃H₁₈O₂ + O₂ → 13 CO₂ + H₂O

Next, we balance the hydrogen by placing a coefficient of 9 in front of H₂O, which gives us 18 hydrogen atoms:

C₁₃H₁₈O₂ + O₂ → 13 CO₂ + 9 H₂O

Now, we calculate the total number of oxygen atoms on the product side. From 13 CO₂, we have 26 oxygen atoms, and from 9 H₂O, we have 9 more, totaling 35 oxygen atoms. Since the reactant side already has 2 oxygen atoms from ibuprofen, we need an additional 33 oxygen atoms from O₂. This requires a coefficient of 16.5 in front of O₂:

C₁₃H₁₈O₂ + 16.5 O₂ → 13 CO₂ + 9 H₂O

To eliminate the fraction, we multiply the entire equation by 2, resulting in whole number coefficients:

2 C₁₃H₁₈O₂ + 33 O₂ → 26 CO₂ + 18 H₂O

This final equation represents the balanced combustion reaction of ibuprofen, illustrating the stoichiometric relationships between the reactants and products involved in the process.

Indicate the type of chemical reaction taking place from the following equation:

• A. Combination
• B. Combustion
• C. Single Displacement
• D. Decomposition

Answer: (C)

Indicate the type of chemical reaction taking place from the following equation:

• A. Decomposition
• B. Double Displacement
• C. Combination
• D. Combustion

Answer: (B)

Indicate the type of chemical reaction taking place from the following equation:

• A. Single Displacement
• B. Combustion
• C. Redox Reaction
• D. Decomposition

Answer: (C)

Here’s what students ask on this topic:

What are the different types of chemical reactions?

Chemical reactions can be categorized into several types based on the changes they undergo and the products formed. The main types include:

• Combination Reactions: Multiple reactants combine to form one product. For example, ${\mathrm{Na}}_{}+{\mathrm{ClO}}_{}\to {\mathrm{NaClO}}_{}$.
• Decomposition Reactions: One reactant breaks down into multiple products. For example, $H_2{O}_{}\to H_2+O_2$.
• Combustion Reactions: Compounds containing carbon and hydrogen react with oxygen to produce water and carbon dioxide. For example, ${\mathrm{CH}}_4+O_2\to {\mathrm{CO}}_2+H_2{O}_{}$.
• Single Displacement Reactions: One element replaces another in a compound. For example, ${\mathrm{Zn}}_{}+{\mathrm{CuSO}}_4\to {\mathrm{ZnSO}}_4+{\mathrm{Cu}}_{}$.
• Double Displacement Reactions: Ions from two compounds swap places. For example, ${\mathrm{Ba(NO}}_3)2+{\mathrm{Na}}_{2_{{\mathrm{SO}}_4}}$.

What is a redox reaction?

A redox reaction, short for reduction-oxidation reaction, involves the transfer of electrons between two species. One reactant undergoes oxidation (loses electrons), while the other undergoes reduction (gains electrons). For example, in the reaction ${\mathrm{Zn}}_{}+{\mathrm{CuSO}}_4\to {\mathrm{ZnSO}}_4+{\mathrm{Cu}}_{}$, zinc is oxidized (loses electrons) and copper is reduced (gains electrons). Redox reactions are essential in various processes, including cellular respiration and combustion.

How can you identify a combustion reaction?

A combustion reaction typically involves a hydrocarbon (a compound containing carbon and hydrogen) reacting with oxygen to produce carbon dioxide and water. The general form of a combustion reaction is $C_{\mathrm{x}}{H}_{\mathrm{y}}+O_2\to {\mathrm{CO}}_2+H_2{O}_{}$. For example, the combustion of methane is ${\mathrm{CH}}_4+O_2\to {\mathrm{CO}}_2+H_2{O}_{}$. Identifying combustion reactions is crucial in understanding energy production and environmental impact.

What is the difference between single displacement and double displacement reactions?

In a single displacement reaction, one element replaces another element in a compound. For example, ${\mathrm{Zn}}_{}+{\mathrm{CuSO}}_4\to {\mathrm{ZnSO}}_4+{\mathrm{Cu}}_{}$, where zinc displaces copper. In contrast, a double displacement reaction involves the exchange of ions between two compounds. For example, ${\mathrm{Ba(NO}}_3)2+{\mathrm{Na}}_{2_{{\mathrm{SO}}_4}}$, where barium and sodium ions swap places. Understanding these differences is essential for predicting reaction products and mechanisms.

How does a decomposition reaction differ from a combination reaction?

A decomposition reaction involves a single reactant breaking down into multiple products. For example, $H_2{O}_{}\to H_2+O_2$, where water decomposes into hydrogen and oxygen gases. In contrast, a combination reaction involves multiple reactants combining to form a single product. For example, ${\mathrm{Na}}_{}+{\mathrm{ClO}}_{}\to {\mathrm{NaClO}}_{}$, where sodium and chlorine combine to form sodium hypochlorite. Recognizing these reaction types helps in understanding chemical processes and predicting reaction outcomes.