Questions: What is the balanced chemical equation for the combustion of methane?

What is the balanced chemical equation for the combustion of methane?
Transcript text: What is the balanced chemical equation for the combustion of methane?
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Solution

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Solution Steps

Step 1: Identify the Reactants and Products

The combustion of methane involves methane (\(\text{CH}_4\)) and oxygen (\(\text{O}_2\)) as reactants. The products of this reaction are carbon dioxide (\(\text{CO}_2\)) and water (\(\text{H}_2\text{O}\)).

Step 2: Write the Unbalanced Equation

The unbalanced chemical equation for the combustion of methane is: \[ \text{CH}_4 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \]

Step 3: Balance the Equation

To balance the equation, ensure that the number of each type of atom is the same on both sides of the equation.

  1. Carbon atoms: There is 1 carbon atom in \(\text{CH}_4\) and 1 in \(\text{CO}_2\). This is already balanced.
  2. Hydrogen atoms: There are 4 hydrogen atoms in \(\text{CH}_4\) and 2 in each \(\text{H}_2\text{O}\). To balance, place a coefficient of 2 in front of \(\text{H}_2\text{O}\): \[ \text{CH}_4 + \text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \]
  3. Oxygen atoms: There are 2 oxygen atoms in \(\text{CO}_2\) and 2 in \(2\text{H}_2\text{O}\), totaling 4 oxygen atoms needed on the product side. Therefore, place a coefficient of 2 in front of \(\text{O}_2\): \[ \text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O} \]

Final Answer

The balanced chemical equation for the combustion of methane is: \[ \boxed{\text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O}} \]

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