The values for the enthalpies of formation of c6h6(l), co2(g) and h2o(l) are 49 kj mol-1, -393 kj mol-1, and -285 kj mol-1 respectively. use this information to determine the enthalpy change when 1 mole of c6h6(l) undergoes combustion to produce carbon dioxide gas and liquid water.

ΔH(Combustion C₆H₆ = -3,262 Kj/mole

Explanation:

hydrocarbons are organic compounds that contain only hydrogens and carbons. they can be saturated (those which contain only carbon-carbon single bonds) or unsaturated (those which contain carbon-carbon double or triple bonds) in nature. hydrocarbons can undergo several reactions like substitution, elimination etc.  

on substituting one or more hydrogen atoms in hydrocarbon it results in the formation of haloalkane. as the halogen atoms are large compared to the carbon and hydrogen atoms, due to which the molecular weight increases and the bond become polar because of presence electronegative halogen atom and results in the increase in boiling point of the haloalkane.

thus, the correct option is (b) that is the boiling point of the new compound increases on substituting a hydrogen atom with a halogen in a hydrocarbon.