The complete combustion of octane, \(\mathrm{C}_{8} \mathrm{H}_{18}\), the main
component of gasoline, proceeds as follows:
$$
2 \mathrm{C}_{8} \mathrm{H}_{18}(l)+25 \mathrm{O}_{2}(g) \longrightarrow 16
\mathrm{CO}_{2}(g)+18 \mathrm{H}_{2} \mathrm{O}(g)
$$
(a) How many moles of \(\mathrm{O}_{2}\) are needed to burn \(1.25 \mathrm{~mol}\)
of \(\mathrm{C}_{8} \mathrm{H}_{18} ?\)
(b) How many grams of \(\mathrm{O}_{2}\) are needed to burn \(10.0 \mathrm{~g}\)
of \(\mathrm{C}_{8} \mathrm{H}_{18}\) ?
(c) Octane has a density of \(0.692 \mathrm{~g} / \mathrm{mL}\) at \(20^{\circ}
\mathrm{C}\). How many grams of \(\mathrm{O}_{2}\) are required to burn \(1.00\)
gal of \(\mathrm{C}_{8} \mathrm{H}_{18}\) ?