Problem- White gas is a mixture of C5 compounds and C6 compounds. The heavier hydrocarbons in white gas are hexanes (C6H14).
1) How much heat is release during the combustion of 3.00 kg of C6H14?
2) How many grams of C6H14 are needed to heat 1.25 kg of water from 23.5C to 80.5C ? Assume that all of the heat released during combustion is use to heat the water.
3) 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 1.25 kg of water from 23.5C to 80.5C?
Show all steps to describe the solution of above problem