Question

What is the main component of natural gas? Write out the balanced chemical equation illustrating its combustion.

Short answer

Methane is the main component, and its combustion is \( ext{CH}_4 + 2 ext{O}_2 ightarrow ext{CO}_2 + 2 ext{H}_2 ext{O} \).

Step-by-step solution

Identify the Main Component

The main component of natural gas is methane. Methane is a simple hydrocarbon with the chemical formula \( ext{CH}_4 \). It is the primary component, making up about 70-90% of natural gas.

Understand Combustion

Combustion is a chemical reaction that involves a substance reacting with oxygen to produce heat and usually light. For hydrocarbons like methane, this reaction typically produces carbon dioxide and water.

Write the Combustion Equation

The unbalanced chemical equation for the combustion of methane can be written as follows: \[ ext{CH}_4 + ext{O}_2 ightarrow ext{CO}_2 + ext{H}_2 ext{O} \]

Balance the Equation

To balance the equation, ensure that the number of atoms of each element is the same on both sides of the equation. For methane combustion: 1. 1 molecule of methane \( ext{CH}_4 \) has 1 carbon and 4 hydrogen atoms.2. Balance carbon by placing 1 molecule of \( ext{CO}_2 \).3. Balance hydrogen by placing 2 molecules of water \( ext{H}_2 ext{O} \).4. Balance oxygen: 2 in \( ext{CO}_2 \) and 2 in \( ext{H}_2 ext{O} \) require 2 molecules of \( ext{O}_2 \). The balanced equation is: \[ ext{CH}_4 + 2 ext{O}_2 ightarrow ext{CO}_2 + 2 ext{H}_2 ext{O} \]

Key concepts

Natural Gas Composition

Natural gas is a convenient source of energy used in homes and industries across the globe. One of its primary advantages is that it burns more cleanly compared to other fossil fuels. The main component of natural gas is methane (\(\text{CH}_4\)), a simple and efficient hydrocarbon.
Methane is colorless and odorless in its pure state. Once extracted from the earth, it is usually purified to reach a methane composition of 70-90%. Understanding this composition is essential because it dictates combustion behavior and energy output.
Apart from methane, natural gas also contains small amounts of other hydrocarbons such as ethane, propane, butane, and trace gases like carbon dioxide and nitrogen. By converting mostly methane to energy, natural gas is a vital and lesser-polluting fuel source in the shift toward more sustainable energy practices.

Chemical Reaction Balancing

Chemical reaction balancing is a crucial concept in chemistry to ensure that the law of conservation of mass is upheld. In a balanced chemical equation, the number of atoms for each element is the same on both sides of the equation.
When balancing a combustion equation like that of methane, start by counting the number of atoms in the reactants and products. Methane has one carbon and four hydrogen atoms. Consequently, it forms one carbon dioxide molecule (\(\text{CO}_2\)) and two water molecules (\(\text{H}_2\text{O}\)).
Here's a simple guide to balance any equation:

• Write the unbalanced equation.
• Start by balancing the atoms of elements that only appear in one reactant and one product.
• Adjust coefficients to get equal numbers of each type of atom on both sides.
• Verify that the total number of each type of atom is equal on both sides.

Balancing chemical equations connects dynamics like stoichiometry to tangible outcomes like energy production.

Carbon Dioxide Production

Carbon dioxide (\(\text{CO}_2\)) is one product of the combustion of hydrocarbons like methane. This gas is naturally present in Earth's atmosphere and plays crucial roles in various biological and chemical processes. However, human activities such as fossil fuel combustion significantly increase its concentration in the atmosphere.
In the balanced combustion reaction of methane:\[ \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O}\] One molecule of methane reacts with two molecules of oxygen to produce one molecule of carbon dioxide, along with water.
It's essential to understand that increasing levels of carbon dioxide contribute to global climate change. Thus, balancing the need for energy with environmental considerations is increasingly vital.

Hydrocarbon Combustion

Hydrocarbon combustion refers to the reaction of hydrocarbons with oxygen to produce energy, alongside by-products like carbon dioxide and water. Methane, being the simplest hydrocarbon, is an excellent example to understand this process.
In combustion, methane (\(\text{CH}_4\)) combines with oxygen (\(\text{O}_2\)) under the right conditions to form carbon dioxide (\(\text{CO}_2\)) and water (\(\text{H}_2\text{O}\)), releasing energy in the form of heat and light. This reaction has the balanced equation:\[\text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O}\]Common characteristics of hydrocarbon combustion are:

• Heat and light as primary energy output.
• Production of carbon dioxide and water as major by-products.
• Potential for incomplete combustion, leading to carbon monoxide or soot.

Hydrocarbon combustion is critical in energy production but requires careful management to reduce environmental impact.