Problem 26 - Chemistry and Chemical Reactivity

Question

Write a balanced equation for the reaction of sulfur trioxide with water.

Step-by-Step Solution

Answer

The balanced equation is SO₃ + H₂O → H₂SO₄.

Step 1: Identify the reactants and products

The problem involves sulfur trioxide and water as reactants. When sulfur trioxide (SO₃) reacts with water (H₂O), it forms sulfuric acid (H₂SO₄) as the product.

Step 2: Write the unbalanced chemical equation

The unbalanced equation for the reaction is: \[ \text{SO}_3 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_4 \] This represents the combination of sulfur trioxide and water to yield sulfuric acid.

Step 3: Balance the chemical equation

To balance the equation, ensure the number of each type of atom is the same on both sides of the equation. We start with the unbalanced equation: \[ \text{SO}_3 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_4 \] Count the number of sulfur (S), oxygen (O), and hydrogen (H) atoms on each side:- Left Side: 1 sulfur, 3 + 1 = 4 oxygen, 2 hydrogen- Right Side: 1 sulfur, 4 oxygen, 2 hydrogen Since the number of each atom type is the same on both sides, the equation is balanced as written.

Key Concepts

Sulfur Trioxide

Sulfur trioxide, often written as \( \text{SO}_3 \), is a chemical compound that plays a vital role in industrial processes. It is a colorless liquid that fumes when exposed to air due to its high affinity for water. An interesting fact about sulfur trioxide is that it readily reacts with water despite its simple molecular structure.

• **Chemical Composition**: It consists of sulfur and oxygen atoms arranged in a triangular planar configuration.
• **Properties**: Being an oxidant, \( \text{SO}_3 \) is highly reactive, especially with water, making it crucial in synthesizing sulfuric acid.
• **Environmental Impact**: Released into the atmosphere, it can form acid rain by reacting with moisture, which is harmful to ecosystems.

Sulfur trioxide's interaction with water underlines its importance in chemical manufacturing, particularly in creating sulfuric acid, which we'll explore further in the next section.

Sulfuric Acid

Sulfuric acid, expressed as \( \text{H}_2\text{SO}_4 \), is one of the most widely used chemicals in industry. It is a strong acid known for its ability to dissolve many substances and its extensive use in fertilizer production.

• **Formation**: This powerful acid forms when sulfur trioxide reacts with water, as shown in the chemical equation: \( \text{SO}_3 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_4 \).
• **Characteristics**: It is a dense, oily liquid that is colorless and odorless. Due to its high boiling point and ability to attract water, it is also called a "dehydrating agent."
• **Industrial Uses**: Besides being used in fertilizers, sulfuric acid is essential in manufacturing chemicals, refining petroleum, and even in metal processing.

Understanding sulfuric acid's properties and roles in industrial processes highlights its indispensability for modern industry.

Chemical Reactions

Chemical reactions are processes where substances, known as reactants, transform into different substances called products. Balancing chemical equations ensures that the law of conservation of mass holds, meaning matter is neither created nor destroyed.

• **Balancing Equations**: It requires counting the number of atoms of each element in reactants and products to ensure they are the same on both sides. For example, in the given equation: \( \text{SO}_3 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_4 \), the balance is achieved as there is one sulfur, four oxygen, and two hydrogen atoms on both sides.
• **Reaction Types**: Reactions like these, where two compounds form a new compound, are known as synthesis reactions.
• **Significance**: Balancing equations is critical for predicting the amount of substances consumed and produced in a reaction.

Ensuring a balanced chemical equation not only respects fundamental scientific laws but also aids in understanding the stoichiometry and dynamics of chemical processes.