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 step by step, we will follow these steps:

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the combustion of isobutane `(C₄H₁₀)` is:
\[ 2C₄H₁₀(g) + 13O₂(g) \rightarrow 8CO₂(g) + 10H₂O(g) \]

### Step 2: Determine the volume of CO₂ produced from the given volume of isobutane
From the balanced equation, we see that 2 moles of isobutane produce 8 moles of carbon dioxide. Therefore, the ratio of isobutane to carbon dioxide is:
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