The boiling points for a set of compounds in a homologous series can be qualitatively predicted using intermolecular force strengths. Using their condensed structural formulas, rank the homologous series for a set of alkanes by their boiling point.

Rank from highest to lowest boiling point. To rank items as equivalent, overlap them.
a)CH3CH2CH2CH3 b) CH3CH2CH2CH2CH2CH3
CH3
c) CH3CH2CCH2CH3
CH3

d)CH3CH2CH2CH2CH2CH2CH3

The given question is incomplete. The complete question is as follows.

The boiling points for a set of compounds in a homologous series can be qualitatively predicted using intermolecular force strengths. Using their condensed structural formulas, rank the homologous series for a set of alkanes by their boiling point.

Rank from highest to lowest boiling point. To rank items as equivalent, overlap them.

butane (), 3,3-dimethylpentane (), hexane (), and heptane ().

Explanation:

It is known that boiling point is the temperature at which vapor pressure of a liquid becomes equal to the atmospheric pressure. In hydrocarbons, more linearly the carbon atoms are attached to each other more will be the boiling point of the compound because of increase in surface area of the compound.

And, more is the branching present in a compound lesser will be its boiling point.

Also, more is the intermolecular strength present in a compound more will be its boiling point.

Thus, we can conclude that given compounds are ranked from highest to lowest boiling point as follows.

          heptane > hexane > 3,3-dimethyl pentane > butane

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

the product of the pressure and volume is also constant