# Question #9245f

Step 2: Now, the density of octane is given as 0.7 g/ml, that is, there are 0.7 grams in 1 ml. This means that there are $0.7 \cdot 11355 = 7948.5 \setminus \setminus \textrm{g r a m s}$ of octane.
Step 3: The molar mass of octane is $114 g$, and so we have $69.72$ moles of octane.
And so, if there is 1,303 kcal of energy from a mole of octane, then there $1303 \setminus \times 69.72 \setminus \approx 90850 \setminus \setminus \textrm{k c a l}$ of energy would be released with 69.72 moles.