Question

The Ostwald process is an industrial method for manufacturing nitric acid. Write three balanced equations for the Ostwald process, starting by heating ammonia and oxygen gases.

Short answer

The balanced equations for the Ostwald process are: 1) \(4\text{NH}_3 + 5\text{O}_2 \to 4\text{NO} + 6\text{H}_2\text{O}\); 2) \(2\text{NO} + \text{O}_2 \to 2\text{NO}_2\); 3) \(3\text{NO}_2 + \text{H}_2\text{O} \to 2\text{HNO}_3 + \text{NO}\).

Step-by-step solution

Balance the Ammonia Oxidation Reaction

The first reaction in the Ostwald process is the oxidation of ammonia (\( ext{NH}_3\) with oxygen (\( ext{O}_2\) to form nitric oxide (\( ext{NO}\) and water (\( ext{H}_2 ext{O}\). The unbalanced equation is: \[ ext{NH}_3 + ext{O}_2 ightarrow ext{NO} + ext{H}_2 ext{O} \]To balance it, we need to ensure that the number of each type of atom is the same on both sides: \(4 ext{NH}_3 + 5 ext{O}_2 ightarrow 4 ext{NO} + 6 ext{H}_2 ext{O}\)

Balance the Nitric Oxide Oxidation Reaction

In this step, we convert nitric oxide (\( ext{NO}\) to nitrogen dioxide (\( ext{NO}_2\) by reacting it with oxygen (\( ext{O}_2\). The unbalanced equation is: \[ ext{NO} + ext{O}_2 ightarrow ext{NO}_2 \]Balancing the equation results in:\[2 ext{NO} + ext{O}_2 ightarrow 2 ext{NO}_2\]

Balance the Formation of Nitric Acid Reaction

Finally, nitrogen dioxide (\( ext{NO}_2\) reacts with water (\( ext{H}_2 ext{O}\) to form nitric acid (\( ext{HNO}_3\) and nitrogen monoxide (\( ext{NO}\). The unbalanced equation is: \[ ext{NO}_2 + ext{H}_2 ext{O} ightarrow ext{HNO}_3 + ext{NO} \]Balancing gives:\[3 ext{NO}_2 + ext{H}_2 ext{O} ightarrow 2 ext{HNO}_3 + ext{NO}\]

Key concepts

Industrial Chemistry: The Ostwald Process

Industrial chemistry plays a vital role in modern manufacturing, transforming raw materials into valuable products. One of the classic processes utilized in this field is the Ostwald process. This particular method is predominantly used to produce nitric acid, an essential component in fertilizers, explosives, and other chemicals.

The Ostwald process begins with the catalytic oxidation of ammonia, which is a derivative of natural gas. This process involves three main chemical reactions that convert ammonia and oxygen into nitric acid. Each reaction involves a catalyst, typically platinum or rhodium, to increase efficiency and speed up the oxidation process.

The success of industrial chemistry processes like the Ostwald process lies in their ability to produce vast quantities of chemicals while minimizing resources and maximizing efficiency. These processes are crucial for meeting global demands in agriculture and various industries.

Understanding Chemical Equations

Chemical equations are representations of chemical reactions showing the reactants and the products. In the Ostwald process, the chemical equations depict how ammonia and oxygen are converted into nitric acid. Each equation must reflect the law of conservation of mass, meaning the number of each type of atom must remain constant on both sides of the equation.

**Key Components of Chemical Equations:**

• **Reactants:** The starting substances which undergo change (e.g., ammonia and oxygen in the Ostwald process).
  
• **Products:** The new substances formed from the reaction (e.g., nitric oxide, nitrogen dioxide, and nitric acid).
  
• **Coefficients:** Numbers placed in front of molecules to balance the equation, ensuring the atom count is equal on both sides.
  
• **States of Matter:** Provided as indicators such as solid \(s\), liquid \(l\), gas \(g\), and aqueous \(aq\).
  

Understanding and writing chemical equations accurately is crucial for predicting the outcomes of chemical reactions.

Balancing Reactions in the Ostwald Process

Balancing reactions is a fundamental skill in chemistry, essential for solving stoichiometry problems and ensuring accurate representations of chemical processes. The Ostwald process serves as an excellent example of how to balance various chemical reactions.

In the first step, the oxidation of ammonia, the unbalanced equation is initially presented, followed by the steps taken to balance it. Each reaction in the Ostwald process requires precise balancing:

• **Ammonia Oxidation:** The balanced equation is \(4 \text{NH}_3 + 5 \text{O}_2 \rightarrow 4 \text{NO} + 6 \text{H}_2\text{O}\). The coefficients are carefully adjusted to maintain the same number of nitrogen, hydrogen, and oxygen atoms on both sides.
  
• **Nitric Oxide Oxidation:** For this reaction, the balanced equation becomes \(2 \text{NO} + \text{O}_2 \rightarrow 2 \text{NO}_2\), ensuring the continuity of the nitrogen and oxygen count.
  
• **Formation of Nitric Acid:** The process finishes with \(3 \text{NO}_2 + \text{H}_2\text{O} \rightarrow 2 \text{HNO}_3 + \text{NO}\). Here, the precise balancing allows for the transformation of nitrogen dioxide and water into nitric acid and nitrogen monoxide.
  

Successfully balancing these equations is crucial for accurately modeling the industrial production of nitric acid.