Number of moles of oxygen requiredfor complete combussion of one mole of pentane is ….......

Answer

To determine the number of moles of oxygen required for the complete combustion of one mole of pentane (C5H12), we can follow these steps:

### Step 1: Write the balanced chemical equation for the combustion of pentane.
The general reaction for the combustion of a hydrocarbon (C_xH_y) is:
\[ \text{C}_x\text{H}_y + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \]

For pentane (C5H12), the balanced equation is:
\[ \text{C}_5\text{H}_{12} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \]

### Step 2: Determine the products of the reaction.
When pentane combusts completely, it produces carbon dioxide (CO2) and water (H2O).

### Step 3: Balance the equation.
1. **Carbon atoms**: Pentane has 5 carbon atoms, so we need 5 CO2 molecules.
2. **Hydrogen atoms**: Pentane has 12 hydrogen atoms, so we need 6 H2O molecules (since each water molecule has 2 hydrogen atoms).
3. **Oxygen atoms**: Now we count the total number of oxygen atoms needed:
- From 5 CO2, we get \(5 \times 2 = 10\) oxygen atoms.
- From 6 H2O, we get \(6 \times 1 = 6\) oxygen atoms.
- Total oxygen atoms needed = \(10 + 6 = 16\) oxygen atoms.

Since O2 has 2 oxygen atoms per molecule, we need:
\[ \frac{16}{2} = 8 \text{ moles of } O_2 \]

### Final Balanced Equation:
The complete balanced equation for the combustion of pentane is:
\[ \text{C}_5\text{H}_{12} + 8 \text{O}_2 \rightarrow 5 \text{CO}_2 + 6 \text{H}_2\text{O} \]

### Step 4: Conclusion
Thus, the number of moles of oxygen required for the complete combustion of one mole of pentane is **8 moles**.

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