The standard heats of formation of `CH_(4)(g), CO_(2)(g)` and `H_(2)O(g)` are `-76.0, -390.0`, and `-240.0 kJ mol^(-1)`, respectively. Calculate the amount of heat evolved by burning `1m^(3)` of methane measured under normal conditions.

Explanation

To solve the problem of calculating the amount of heat evolved by burning 1 m³ of methane (CH₄) under normal conditions, we can follow these steps:

### Step 1: Write the balanced chemical equation for the combustion of methane.
The balanced equation for the combustion of methane is:
\[ \text{CH}_4(g) + 2 \text{O}_2(g) \rightarrow \text{CO}_2(g) + 2 \text{H}_2\text{O}(g) \]

### Step 2: Identify the standard heats of formation.
From the problem, we have the following standard heats of formation:
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