Ethane burns in oxygen by the following equation:
`2C_(2)H_(6)+7O_(2) rarr 4CO_(2) + 6H_(2)O`
2.5L of ethane are burnt in excess of oxygen at `27^(@)C` and 1 atm pressure. Calculate how many litres of `CO_(2)` are formed.
at `27^(@)C` and 1.0 atm?

Explanation

To solve the problem of how many liters of \( CO_2 \) are formed when 2.5 L of ethane is burned, we can follow these steps:

### Step 1: Write down the balanced chemical equation
The balanced chemical equation for the combustion of ethane is:
\[ 2C_2H_6 + 7O_2 \rightarrow 4CO_2 + 6H_2O \]

### Step 2: Determine the stoichiometric ratio
From the balanced equation, we can see that:
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