The combustion of octane is expressed by the thermochemical equation

Estimate the mass of octane that would need to be burned to produce enough heat to raise the temperature of the air in a 12 ft * 12 ft * 8.0 ft room from 40.°F to 78 °F on a mild winter’s day. 

(a) Use the normal composition of air to determine its density and assume a pressure of 1.00 atm.

(b) How much heat will be evolved from the combustion of 1.0 gallon of gasoline (assumed to be exclusively octane)? The density of octane is 0.70 g · mL^–1.

Transcribed Image Text:

C8H18 (1) + 0₂(g) 8 CO₂ (g) +9 H₂O (1) AH° -5471 kJ