Chapter 10, Problem 67E

What mass in grams of octane, a component of gasoline, would you have to burn in your car to transfer $9.48\times {10}^5\text{kJ}$ of energy? ${\Delta }_{\text{f}}\text{H}=-1.09\times {10}^4\text{kJ}$ for the reaction ${\text{2C}}_{\text{8}}{\text{H}}_{\text{18}}\left(l\right)+{\text{25O}}_{\text{2}}\left(\text{g}\right)\to 16{\text{CO}}_{\text{2}}\left(\text{g}\right)+18{\text{H}}_{\text{2}}\text{O}\left(l\right)$?