The molar heat of combustion of pentan-1-ol, C5H11OH, is 3329 kJ mol⁻¹ - VCE - SSCE Chemistry - Question 25 - 2018 - Paper 1

Using the molar heat of combustion, the number of moles required can be calculated:

$n = \frac{\text{Energy}}{\text{Molar Heat of Combustion}} = \frac{10800000 ext{ kJ}}{3329 ext{ kJ mol}^{-1}} \approx 3243.52 ext{ mol}$

Now calculate the mass using the molar mass of C5H11OH:

$\text{mass} = n \times M = 3243.52 ext{ mol} \times 88.0 ext{ g mol}^{-1} \approx 285395.76 ext{ g}$

Finally, convert grams to tonnes (1 tonne = 1000 kg = 1000000 g):

$\text{mass in tonnes} = \frac{285395.76 ext{ g}}{1000000} \approx 0.2854 ext{ tonnes}$

The closest answer to the calculated value of approximately 0.286 tonnes is:

B. 0.286