Ethanol (c2h5oh) is currently blended with gasoline as an automobile fuel. calculate the heat produced per liter of ethanol by combustion of ethanol under constant pressure. ethanol has a density of 0.789 g/ml.

-2.34 × 10⁴ kJ/L

Explanation:

Let's consider the reaction for the combustion of ethanol.

C₂H₅OH(l) + O₂(g) ⇒ CO₂(g) + H₂O(l)

The enthalpy of combustion (heat rteleased under constant pressure) of ethanol is -1366.8 kJ/mol. Considering the molar mass of ethanol is 46.07 g/mol, the heat produced per liter of ethanol is:

substituting a hydrogen atom with a halogen in a hydrocarbon:

- the single bond remains single. a is wrong.

- the bond with hydrogen is as strong as with a halogen. c is wrong

- a hydrocarbon is saturated if there is no double bond. we do not know that so d is wrong.

- carbon will always have four valence electrons. e is wrong.

by elimination, the correct answer is b. the boiling point of the new compound increases.