Which of the following is the correct equation for an INCOMPLETE combustion of octane? (A) $C_8H_{18}(l) + 8O_2(g) \rightarrow 8CO_2(g) + 9H_2(g)$ (B) $C_8H_{18}(l) + \frac{25}{2} O_2(g) \rightarrow 8CO_2(g) + 9H_2O(l)$ (C) $C_8H_{18}(l) + 6O_2(g) \rightarrow 3CO(g) + 5H_2O(l)$ (D) $C_8H_{18}(l) + 13O_2(g) \rightarrow 4CO(g) + 4C(s) + 9H_2O(l)$ - HSC - SSCE Chemistry - Question 7 - 2013 - Paper 1

The process of incomplete combustion of octane involves the reaction of octane ($C_8H_{18}$) with oxygen ($O_2$), resulting in the production of carbon monoxide ($CO$) and water ($H_2O$) instead of carbon dioxide ($CO_2$).

Among the given options, option (C) is:

$C_8H_{18}(l) + 6O_2(g) \rightarrow 3CO(g) + 5H_2O(l)$

This equation reflects incomplete combustion, where not all carbon from octane is converted to carbon dioxide, resulting in carbon monoxide as a product.