Isobutane `(C_(4)H_(10))` undergoes combustion in oxygen according to the following reaction:
`2C_(4)H_(10)(g)+13O_(2)(g) rarr 8CO_(2)(g)+10H_(2)O(e)`
When `10.00 L` of isobutane is burnt at `27^(@)C` and `1 bar` pressure, calculate the volume of `CO_(2)` produced at `120^(@)C` and `4.0 bar` pressure.

Explanation

To solve the problem of calculating the volume of CO₂ produced from the combustion of isobutane (C₄H₁₀), we can follow these steps:

### Step 1: Determine the volume of CO₂ produced at initial conditions
The balanced chemical equation for the combustion of isobutane is:
\[ 2C_{4}H_{10}(g) + 13O_{2}(g) \rightarrow 8CO_{2}(g) + 10H_{2}O(l) \]

From the equation, we can see that 2 volumes of isobutane produce 8 volumes of CO₂. Therefore, the ratio of isobutane to CO₂ is:
\[ \frac{8 \text{ L CO₂}}{2 \text{ L C₄H₁₀}} = 4 \text{ L CO₂ per L C₄H₁₀} \]
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