Complete combusion of `CH_(4)` gives :

Options

A. `CO_(2)+H_(2)O`
B. `CO_(2)+H_(2)`
C. `COCl_(2)`
D. `CO+CO_(2) + H_(2)O`

Explanation

To determine the products of the complete combustion of methane (CH₄), we can follow these steps:

### Step 1: Write the chemical equation for complete combustion.
The complete combustion of hydrocarbons involves reacting with oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O). The general equation for the complete combustion of a hydrocarbon (CnH₂n+2) is:

\[ \text{CnH}_{2n+2} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \]

### Step 2: Identify the components for methane (CH₄).
For methane, which is CH₄, we can identify:
- C = 1 (1 carbon atom)
- H = 4 (4 hydrogen atoms)

### Step 3: Write the balanced equation.
The balanced equation for the complete combustion of methane is:

\[ \text{CH}_4 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \]

### Step 4: Balance the equation.
1. **Carbon Balance**: There is 1 carbon atom in CH₄, so we need 1 CO₂:
\[ \text{CH}_4 + \text{O}_2 \rightarrow 1 \text{CO}_2 + \text{H}_2\text{O} \]

2. **Hydrogen Balance**: There are 4 hydrogen atoms in CH₄, so we need 2 H₂O:
\[ \text{CH}_4 + \text{O}_2 \rightarrow 1 \text{CO}_2 + 2 \text{H}_2\text{O} \]

3. **Oxygen Balance**: Now we count the oxygen atoms on the right side:
- From CO₂: 2 oxygen atoms
- From 2 H₂O: 2 × 1 = 2 oxygen atoms
- Total = 2 + 2 = 4 oxygen atoms

Therefore, we need 4 oxygen atoms from O₂, which means we need 2 O₂ molecules:
\[ \text{CH}_4 + 2 \text{O}_2 \rightarrow 1 \text{CO}_2 + 2 \text{H}_2\text{O} \]

### Final Balanced Equation:
The complete balanced equation for the combustion of methane is:
\[ \text{CH}_4 + 2 \text{O}_2 \rightarrow \text{CO}_2 + 2 \text{H}_2\text{O} \]

### Step 5: Identify the products.
From the balanced equation, we can see that the complete combustion of methane (CH₄) produces:
- Carbon dioxide (CO₂)
- Water (H₂O)