White gas is a mixture of C5 compounds and C6 compounds. The heavier hydrocarbons in white gas are hexanes (C6H14).
Given that delta H combustion = -4163 kJ/mol, the fuel value of C6H14 is 48.31 kJ/g and the amount of heat released during the combustion of 5.00 kg of C6H14 is 241,550 kJ. Assuming that all of the heat released during the combustion is used to heat the water, 4.61 grams of C6H14 are needed to heat 1.00 kg of water from 29.5 degrees celsius to 77.5 degrees celsius.
a. Assume white gas is 25% C5 hydrocarbons (fuel value=48.99 kJ/g) and 75% C6 hydrocarbons. How many grams of white gas are needed to heat 1.00 kg of water from 29.5 degrees celsius to 77.5 degrees celsius?