During the combustion of 5.00 g of octane, C8H18, 239.5 kcal (1002 kJ) is released. How much energy (in kJ) is released by the combustion of 1.49 mol of C8H18 ?

Thank you sooo much!!!!

That’s incorrect

To find the amount of energy released by the combustion of 1.49 mol of C8H18, we need to use the given information about the energy released in the combustion of 5.00 g of C8H18.

First, we calculate the molar mass of C8H18:
C: 12.01 g/mol * 8 atoms = 96.08 g/mol
H: 1.01 g/mol * 18 atoms = 18.18 g/mol

Total molar mass of C8H18 = 96.08 g/mol + 18.18 g/mol = 114.26 g/mol

Next, we calculate the amount of energy released by the combustion of 5.00 g of C8H18:

239.5 kcal/g * 5.00 g = 1197.5 kcal

To convert kcal to kJ, we use the conversion factor: 1 kcal = 4.184 kJ

1197.5 kcal * 4.184 kJ/kcal = 5009.41 kJ

So, the combustion of 5.00 g of C8H18 releases 5009.41 kJ of energy.

Now, we can use this information to calculate the amount of energy released by the combustion of 1.49 mol of C8H18:

1.49 mol * (5009.41 kJ / 5.00 g) = 1490.64 kJ

Therefore, the combustion of 1.49 mol of C8H18 releases 1490.64 kJ of energy.

molar mass C8H18 = approx 114 but you should confirm that.

grams = mols x molar mass = 1.49 mols x 114 g/mol = approx 170. Again, you need a better numb er than that estimate. Then
1002 kJ x (170 g/5.00 g) = ? kJ.