# Assuming that gasoline is C8H18 and has a density of 0.703 g/ml, how many liters of CO2 will be produced from the consumption of 1.8 gallons of gasoline at standard conditions ?

${C}_{8} {H}_{18} \left(l\right) + \frac{25}{2} {O}_{2} \left(g\right) \rightarrow 8 C {O}_{2} \left(g\right) + 9 {H}_{2} O \left(g\right)$
Is the equation above stoichiometrically balanced? (And what does stoichiometric mean?). This equation tells us that for each mole of octane (each 116 g!), 8 moles of carbon dioxide ($8 \times 44 \cdot g$) will result. Now the question tells us that 1.8 gallons of gas have been consumed.