🤓 Based on our data, we think this question is relevant for Professor Saykally's class at CAL.

**Determine the moles of CO _{2} first**

${\mathbf{n}}_{{\mathbf{CO}}_{\mathbf{2}}}\mathbf{=}\mathbf{402}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{C}}_{\mathbf{8}}{\mathbf{H}}_{\mathbf{18}}}\mathbf{\left(}\frac{\mathbf{16}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{CO}}_{\mathbf{2}}}{\mathbf{2}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{C}}_{\mathbf{8}}{\mathbf{H}}_{\mathbf{18}}}}\mathbf{\right)}\mathbf{=}$**3216 mol CO**_{2}

**Now we have the number of ****moles CO _{2} produced**

The combustion of octane, C_{8}H_{18}, proceeds according to the reaction:

2 C_{8}H_{18}(l) + 25 O_{2}(g) → 16 CO_{2}(g) + 18 H_{2}O(l)

If 402 mol of octane combusts, what volume of carbon dioxide is produced at 14.0 °C and 0.995 atm?