Hot can
Hot food or beverages prepared without external heat
Termite reaction
Welding of railway tracks
Combustion of fuel
Used for cooking food
Gel pads
Relieves fever
Self cooling beverages
Beverages in cold cans without storing in refrigerators or using ice
Sorbet
The tongue feels cold when the sorbet is put in the mouth
Question
The heat of combustion of octane, \(C_8H_{18}\) is \(-5\,500 \text{ kJ mol}^{−1}\).
Calculate the fuel value of octane, \(C_8H_{18}\).
[Relative atomic mass: H = 1, C = 12]
Solution
Molar mass of octane, \(C_8H_{18}\).
\(=(8 \times 12)+(18 \times1)\\ =96+18\\ =114\text{ g mol}^{−1}\)
Complete combustion of 114 g of octane, \(C_8H_{18}\) releases 5 500 kJ of heat.
Therefore, combustion of 1 g of octane, \(C_8H_{18}\) is as follows;
\(=\dfrac{5\,500 \text{ kJ mol}^{−1}}{114 \text{ g mol}^{−1}}\\ =48.2\text{ kJ g}^{−1}\)
The fuel value of octane, \(C_8H_{18}\) is \(48.2\text{ kJ g}^{−1}\).
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