`CH_(4)(g) +2O_(2)(g) rarr CO_(2)(g) +2H_(2)O(l), DeltaH =- 890 kJ`
what is the calorific or fuel value of `1kg` of `CH_(4)`?

Explanation

To find the calorific or fuel value of 1 kg of methane (CH₄), we can follow these steps:

### Step 1: Understand the Reaction
The combustion of methane can be represented by the equation:
\[ \text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2\text{O}(l) \]
The enthalpy change (ΔH) for this reaction is given as -890 kJ. This means that when 1 mole of methane is burned, it releases 890 kJ of energy.

### Step 2: Calculate the Molar Mass of Methane
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