Calculate the heat produced when `3.785 L` of octabe reacts with oxygeb to form carbon mono oxide and water vapour at `25^(@)C`. (Density of octane is `0.75025 g mL^(-1)). Delta_(comb)H^(Theta)(C_(8)H_(18)) =- 1302.7 kcal, Delta_(f)H^(Theta) (CO_(2)) =- 94.05 kcal, Delta_(f)H^(Theta) (H_(2)O) =- 64.32 kcal, Delta_(f)H^(Theta) (CO) =- 26.41 kcal mo^(-1)`

Explanation

To calculate the heat produced when 3.785 L of octane reacts with oxygen to form carbon monoxide and water vapor at 25°C, we will follow these steps:

### Step 1: Calculate the number of moles of octane (C₈H₁₈)

1. **Convert volume from liters to milliliters**:
\[ \text{Volume in mL} = 3.785 \, \text{L} \times 1000 \, \text{mL/L} = 3785 \, \text{mL} \]
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