Question

Give examples of two acidic oxides. Write equations illustrating the formation of each oxide from its component elements. Write another chemical equation that illustrates the acidic character of each oxide.

Short answer

Examples are CO₂ and SO₃; they form acids H₂CO₃ and H₂SO₄ with water.

Step-by-step solution

Identify Two Acidic Oxides

Acidic oxides are oxides of non-metals that react with water to form acids or with bases to form salts. Two common examples of acidic oxides are carbon dioxide (CO₂) and sulfur trioxide (SO₃).

Formation Equation for Carbon Dioxide

Carbon dioxide is formed when carbon (C) burns in the presence of oxygen (O₂). The chemical equation for this reaction is:\[ \text{C (s) + O}_2 \text{ (g) } \rightarrow \text{ CO}_2 \text{ (g)} \]

Demonstrate Acidic Character of Carbon Dioxide

When carbon dioxide reacts with water, it forms carbonic acid (H₂CO₃). The chemical reaction is:\[ \text{CO}_2 \text{ (g) + H}_2\text{O (l) } \rightarrow \text{ H}_2\text{CO}_3 \text{ (aq)} \]

Formation Equation for Sulfur Trioxide

Sulfur trioxide is formed when sulfur dioxide (SO₂) reacts with oxygen. This process usually occurs with a catalyst in industrial processes. The equation is:\[ \text{2 SO}_2 \text{ (g) + O}_2 \text{ (g) } \rightarrow \text{ 2 SO}_3 \text{ (g)} \]

Demonstrate Acidic Character of Sulfur Trioxide

Sulfur trioxide reacts with water to form sulfuric acid (H₂SO₄), illustrating its acidic nature. The chemical equation is:\[ \text{SO}_3 \text{ (g) + H}_2\text{O (l) } \rightarrow \text{ H}_2\text{SO}_4 \text{ (aq)} \]

Key concepts

Carbon Dioxide

Carbon dioxide, often abbreviated as CO₂, is a gas that plays significant roles in ecosystems and chemical processes. It is naturally occurring as it is a part of the Earth's atmosphere. It can also be produced through various human activities such as combustion of fossil fuels.
When we talk about acidic oxides, carbon dioxide is a classic example. An acidic oxide can react with water to form acids, and in this case, CO₂ reacts with water to form carbonic acid \(\text{H}_2\text{CO}_3\). This reaction is represented by the chemical equation:\[\text{CO}_2 \text{ (g) + H}_2\text{O (l) } \rightarrow \text{ H}_2\text{CO}_3 \text{ (aq)}\] This acid can further influence environmental and chemical reactions. It helps in the formation of caves through the dissolution of limestone and contributes to ocean acidity.
In terms of its formation, carbon dioxide is produced naturally when carbon sources such as wood or coal burn in the presence of oxygen. The simple equation is \[\text{C (s) + O}_2 \text{ (g) } \rightarrow \text{ CO}_2 \text{ (g)}\]It's essential to understand these reactions and equations to grasp the broader implications of this compound in chemical processes and the environment.

Sulfur Trioxide

Sulfur trioxide, written as SO₃, is another prominent acidic oxide. It is particularly well-known due to its role in the formation of acid rain. This compound is produced in industrial processes, specifically during the production of sulfuric acid, which is an essential chemical in numerous industries.
The formation of sulfur trioxide from sulfur dioxide involves a reaction with oxygen. This can be expressed by the following chemical equation:\[\text{2 SO}_2 \text{ (g) + O}_2 \text{ (g) } \rightarrow \text{ 2 SO}_3 \text{ (g)}\]In this reaction, high temperatures and catalysts such as vanadium pentoxide can be used to facilitate the conversion.
The characteristics of sulfur trioxide as an acidic oxide are demonstrated when it reacts with water to form sulfuric acid \(\text{H}_2\text{SO}_4\). This reaction is crucial because sulfuric acid is highly corrosive and plays a vital role in numerous chemical and manufacturing processes. The chemical equation for this reaction is:\[\text{SO}_3 \text{ (g) + H}_2\text{O (l) } \rightarrow \text{ H}_2\text{SO}_4 \text{ (aq)}\]Understanding this reaction is critical to appreciating how acidic oxides contribute to both industrial applications and environmental issues such as acid rain.

Chemical Equations

Chemical equations are the symbolic representation of chemical reactions. They help us clearly understand how substances interact with each other, forming new products or changing states. Equations are often balanced to ensure the conservation of mass, meaning that the number of atoms of each element is equal on both sides of the equation.
For instance, the formation of carbon dioxide from carbon and oxygen is represented as:\[\text{C (s) + O}_2 \text{ (g) } \rightarrow \text{ CO}_2 \text{ (g)}\]Here, one carbon atom and two oxygen atoms (from one molecule of oxygen gas) combine to form one molecule of carbon dioxide.
Similarly, the combination of sulfur dioxide and oxygen to form sulfur trioxide is given by:\[\text{2 SO}_2 \text{ (g) + O}_2 \text{ (g) } \rightarrow \text{ 2 SO}_3 \text{ (g)}\]This equation ensures that four oxygen atoms and two sulfur atoms on both sides of the equation reflect conservation of mass.
Chemical equations don’t just show how to make substances, they also help us understand the inherent nature and behavior of those substances. They illustrate principles like reaction conditions, state of matter (indicated in parentheses), and stoichiometry which involves the quantification of reactants and products in chemical reactions. Proper understanding of chemical equations is fundamental in studying chemistry and understanding nature's complex processes.