Calculate the heat of vaporization of carbon tetrachloride given that the standard molar enthalpy of formation of liquid carbon tetrachloride is -135.4 kj/mol and the standard molar enthalpy of formation of gaseous carbon tetrachloride is -102.9 kj/mol.
a. +102.9 kj/mol
b. -32.5 kj/mol
c. +238.3 kj/mol
d. +32.5 kj/mol
e. -238.3 kj/mol

why is the answer d? for any

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 answer is the first option

explanation:

just googled it m8. not that hard

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