A gas mixture of `3.67L` of ethylene and methane on complete combustion at `25^(@)C` produces `6.11 L` of `CO_(2)`. Find out the heat evolved on buring `1L` of the gas mixture. The heats of combustion of ethylene and methane are `-1423` and `-891kJ mol^(-1)`, respectively, at `25^(@)C`.

Explanation

To solve the problem, we need to determine the volume of ethylene (C₂H₄) and methane (CH₄) in the gas mixture, calculate the heat evolved from their combustion, and then find the heat evolved on burning 1 liter of the gas mixture.

### Step-by-Step Solution:

1. **Set Up the Equations:**
Let the volume of ethylene be \( A \) liters and the volume of methane be \( B \) liters. From the problem, we have:
\[
A + B = 3.67 \quad \text{(1)}
...