For the reaction of ethylene represented above, delta H is - 1,323 kJ. What is the value of delta H if the combustion produced liquid water H2O(l), rather than water vapor H2O(g)? (delta H for the phase change H2O(g) -> H2O(l) is -44 kJ mol-1.)

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"

bcde is the incorrect answer it is a

answer: mole of the gas

answer: mole of the gasexplanation: