Problem 68 - Chemistry Principles and Practice

Question

The largest use of nitric acid is in the production of ammonium nitrate. Write the equation for this process.

Step-by-Step Solution

Answer

The chemical equation is \( \text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3 \).

Step 1: Identify the Reactants

The production of ammonium nitrate involves two main components: nitric acid (HNO₃) and ammonia (NH₃). These will be our reactants for the chemical equation.

Step 2: Determine the Reaction Outcome

Ammonium nitrate (NH₄NO₃) is formed when ammonia reacts with nitric acid. Therefore, the products of this reaction are ammonium nitrate itself.

Step 3: Write the Balanced Chemical Equation

The balanced chemical equation for the reaction of nitric acid with ammonia to produce ammonium nitrate is:\[ \text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3 \]Here, each element in the reactants and products is already balanced.

Key Concepts

Nitric Acid

Nitric acid, chemically represented as \( \text{HNO}_3 \), is a strong and highly corrosive mineral acid. It is pivotal in various industrial processes, especially in the production of fertilizers such as ammonium nitrate.
Nitric acid is colorless when pure but often acquires a yellow hue due to decomposition into nitrogen dioxide \((\text{NO}_2)\). It is used in the production of explosives, in nitration processes, and as a powerful oxidizing agent.

• Highly soluble in water
• Strongly acidic and reactive, particularly with bases like ammonia
• Essential in manufacturing fertilizers

The importance of nitric acid in producing ammonium nitrate is critical due to its ability to donate a nitrate ion to ammonia, forming this valuable compound used primarily in agriculture.

Ammonia

Ammonia, with the chemical formula \( \text{NH}_3 \), is a colorless gas with a distinctive pungent smell. It is a key player in various metabolic processes and also serves extensive industrial uses. Ammonia is one of the most produced inorganic chemicals, highlighting its significance in many fields.
Industrially, ammonia is synthesized by combining nitrogen with hydrogen in the Haber-Bosch process. It is a building block for the synthesis of many nitrogen-containing compounds, including fertilizers like ammonium nitrate.

• Basic nature, capable of neutralizing acids
• Valued for its nitrogen content
• Used in cleaning agents and fertilizers

In the context of its reaction with nitric acid, ammonia acts as a base and readily reacts to form ammonium nitrate. This transformation capitalizes on ammonia's ability to receive a proton from nitric acid, forming the ammonium ion \((\text{NH}_4^+)\).

Balanced Equation

A balanced chemical equation ensures that the same number of each type of atom exists in both the reactants and products, thus obeying the law of conservation of mass. For the reaction between nitric acid and ammonia, it’s essential to depict how these substances interact to form ammonium nitrate.
The balanced chemical equation is:\[ \text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3 \]This equation demonstrates that one molecule of ammonia \(\text{NH}_3 \) reacts with one molecule of nitric acid \(\text{HNO}_3\) to yield one molecule of ammonium nitrate \(\text{NH}_4\text{NO}_3\). All the elements involved—nitrogen, hydrogen, and oxygen—are balanced on both sides of the equation.

• Atoms on reactants side = Atoms on products side
• Reflects real-world usage and requirements for safety and efficiency
• Foundational for chemical analysis and design

Balancing equations is a fundamental skill in chemistry, essential for accurately modeling chemical reactions and predicting the products formed.