Question

One mole of either carbon monoxide or benzene are completely combusted with oxygen at constant temperature...

One mole of either carbon monoxide or benzene are completely combusted with oxygen at constant temperature and pressure (298 K and 1 atm) to generate CO2 and H2O. Assume all substances are ideal gases for calculating volume changes.

a. Write out balanced combustion reactions for each reaction.

b. Calculate the change in entropy for the system for each reaction, using the table, below.

c. Use the enthalpies of formation to calculate the heat lost or gained during this reaction.

d. Use your result in part c) to calculate the change in entropy of the surroundings for each reaction.

e. Also calculate ΔU, ΔA, ΔG for the system for each reaction.

f. Which of the four thermodynamic potentials (ΔU, ΔH, ΔA, ΔG) is suited for an experiment at constant T, P when evaluating if the reaction is spontaneous? What if the experiment is conducted in a rigid container at constant temperature?

substance (all gases)

ΔformationHѲ [kJ/mol]

molar entropy SѲ [J K-1 mol-1]
CO(carbon monoxide) -110.5 197.7

C6H6 (benzene)

 82.9 269.3
O2 0 205.1
CO2 -393.5 213.1
H2O -241.8 188.8
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Answer #1

The question is pretty big, please split in two parts, i am solving the first three parts for both the reactions

a)

b)

Entropy for the first reaction = Entropy of CO2 - Entropy of CO - 1/2 * Entropy of O2

=> 213.1 - 197.7 - 205.1/2

=> -87.15 J/Kmol

Entropy for the second reaction = 6 * Entropy of CO2 + 3 * Entropy of H2O - 15/2 * Entropy of O2 - Entropy of C6H6

=> 6 * 213.1 + 3 * 188.8 - 7.5 * 205.1 - 269.3

=> 37.45 J/Kmol

c)

Enthalpy for the first reaction = Enthalpy of CO2 - Enthalpy of CO - 1/2 * Enthalpy of O2

=> -393.5 + 110.5

=> -283 KJ/mol

Enthalpy for the second reaction = 6 * Enthalpy of CO2 + 3 * Enthalpy of H2O - 15/2 * Enthalpy of O2 - Enthalpy of C6H6

=> 6 * (-393.5) + 3 * (-241.8) - 82.9

=> -3169.3 KJ/mol

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