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 is:
\[ \text{Hydrocarbon} + \text{Oxygen} \rightarrow \text{Carbon Dioxide} + \text{Water} \]

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: Balance the carbon atoms.
Pentane has 5 carbon atoms. Therefore, we need 5 moles of carbon dioxide (CO2) produced:
\[ \text{C}_5\text{H}_{12} + \text{O}_2 \rightarrow 5 \text{CO}_2 + \text{H}_2\text{O} \]

### Step 3: Balance the hydrogen atoms.
Pentane has 12 hydrogen atoms. To balance the hydrogen, we need 6 moles of water (H2O) produced (since each water molecule has 2 hydrogen atoms):
\[ \text{C}_5\text{H}_{12} + \text{O}_2 \rightarrow 5 \text{CO}_2 + 6 \text{H}_2\text{O} \]

### Step 4: Balance the oxygen atoms.
Now, we count the oxygen atoms on the right side of the equation:
- From 5 CO2: \(5 \times 2 = 10\) oxygen atoms
- From 6 H2O: \(6 \times 1 = 6\) oxygen atoms
- Total oxygen on the right side: \(10 + 6 = 16\) oxygen atoms

Since oxygen (O2) is diatomic, we need to divide the total number of oxygen atoms by 2 to find the number of moles of O2 required:
\[ \frac{16}{2} = 8 \text{ moles of } O_2 \]

### Final Answer:
The number of moles of oxygen required for the complete combustion of one mole of pentane is **8 moles**.

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