The equation shows one mole of ethanol fuel being burned in oxygen. Convert the energy released into its equivalent mass.
C2 H5 OH (l) + 3 O2 (g) -- 2 CO2 (g) + 3 H2O (l)
deltaH = -1418 kJ/mol

Question

The equation shows one mole of ethanol fuel being burned in oxygen. Convert the energy released into its equivalent mass.
C2 H5 OH (l) + 3 O2 (g) --> 2 CO2 (g) + 3 H2O (l) 
deltaH = -1418 kJ/mol

anonymous · Answer

I really need help with this.

anonymous · Answer

"convert the energy released into its equivalent mass."
is this E=mc^2 or am I completely misunderstanding the question?

jfraser · Answer

you might use E = mC^2 if the question is very general. If, somewhere else in the lab, you have a quantity of energy released by an unknown amount of ethanol, then use the stoichimetric ratio to find the equivalent mass.