Problem 15 - Chemistry and Chemical Reactivity

Question

Write balanced chemical equations for the reaction of hydrogen gas with oxygen, chlorine, and nitrogen.

Step-by-Step Solution

Answer

Balanced equations: \(2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O}\), \(\text{H}_2 + \text{Cl}_2 \rightarrow 2\text{HCl}\), and \(3\text{H}_2 + \text{N}_2 \rightarrow 2\text{NH}_3\).

Step 1: Write Unbalanced Equations

First, write the unbalanced chemical equations for hydrogen reacting with oxygen, chlorine, and nitrogen. These reactions are: \( \text{H}_2 + \text{O}_2 \rightarrow \text{H}_2\text{O} \), \( \text{H}_2 + \text{Cl}_2 \rightarrow \text{HCl} \), and \( \text{H}_2 + \text{N}_2 \rightarrow \text{NH}_3 \).

Step 2: Balance Hydrogen and Oxygen Equation

For the reaction with oxygen, \( \text{H}_2 + \text{O}_2 \rightarrow \text{H}_2\text{O} \), balance the atoms. We have 2 H in \( \text{H}_2 \) and 2 in two molecules of \( \text{H}_2\text{O} \). Thus, the balanced equation becomes \( 2\text{H}_2 + \text{O}_2 \rightarrow 2\text{H}_2\text{O} \).

Step 3: Balance Hydrogen and Chlorine Equation

For the reaction with chlorine, \( \text{H}_2 + \text{Cl}_2 \rightarrow \text{HCl} \), we need equal numbers of hydrogen and chlorine atoms on each side. Therefore, it becomes \( \text{H}_2 + \text{Cl}_2 \rightarrow 2\text{HCl} \).

Step 4: Balance Hydrogen and Nitrogen Equation

For the reaction with nitrogen, \( \text{H}_2 + \text{N}_2 \rightarrow \text{NH}_3 \), notice that we need 3 hydrogen molecules to get 6 H atoms (as found in 2 \( \text{NH}_3 \)). Balance to get \( 3\text{H}_2 + \text{N}_2 \rightarrow 2\text{NH}_3 \).

Key Concepts

Chemical Reactions

Chemical reactions are processes where substances called reactants are transformed into different substances known as products. These reactions involve the breaking and forming of chemical bonds, leading to a change in the molecular structure. In simple terms, it's how substances interact to create something entirely new.

• Reactants: The starting substances in a chemical reaction.
• Products: The new substances made by the reaction.
• Molecular Changes: Chemical bonds in the reactants are broken and reformed to create products.

Writing a chemical equation is a way to describe this transformation using chemical formulas. An equation consists of reactants on the left-hand side and products on the right-hand side, separated by an arrow (→). For example, in the reaction of hydrogen with oxygen, hydrogen (\( \text{H}_2 \)) and oxygen (\( \text{O}_2 \)) are reactants that form water (\( \text{H}_2\text{O} \)) as the product.

Hydrogen Reactions

Hydrogen, the lightest and most abundant element in the universe, is extremely reactive. It easily forms compounds with a wide range of other elements. In reactions, hydrogen molecules (\( \text{H}_2 \)) typically act as reducing agents, helping other substances to gain electrons.When hydrogen reacts, distinct products are formed based on the reacting partner. Here are some examples:

• With Oxygen: Produces water (\( \text{H}_2 + \text{O}_2 \rightarrow \text{H}_2\text{O} \)), a fundamental component for life.
• With Chlorine: Produces hydrogen chloride gas (\( \text{H}_2 + \text{Cl}_2 \rightarrow \text{HCl} \)), which dissolves in water to form hydrochloric acid.
• With Nitrogen: Produces ammonia (\( \text{H}_2 + \text{N}_2 \rightarrow \text{NH}_3 \)), a key ingredient in fertilizers.

Balancing these reactions involves ensuring the same number of each type of atom on both sides of the equation. This keeps the mass unchanged, respecting the law of conservation of mass.

Molecular Equations

Molecular equations represent the reactants and products in a chemical reaction using their molecular formulas. They provide a clear snapshot of the molecules involved in the reaction, showing the actual compounds rather than the ions present in a solution. Molecular equations are key in describing reactions because they:

• Help in visualizing how substances interact during a chemical process.
• Convey stoichiometric relationships, showing the precise amount of reactants needed to produce a specific amount of product.
• Aid in balancing chemical equations, ensuring that atoms are conserved during the reaction.

For instance, when balancing hydrogen's reaction with nitrogen, the molecular equation is \( \text{3H}_2 + \text{N}_2 \rightarrow \text{2NH}_3 \). This represents the precise rearrangement of atoms and molecules, essential for understanding the reaction dynamics.