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Free energy change of a reaction

Consider the combustion reaction for propane below.
CH3CH2CH3(g)+5O2(g)-------->3 C02(g)+4H20(g)

a) Determine the delta G standard state at 298 K from the following standard state values at T= 298
S(CH3CH2CH3)=269.9 J/K mol
S(C02)= 213.7 J/K mol
S(H20)=188.8 J/K mol
S(02)=205.1 J/ K mol
delta H(CH3CH2CH3)=-103.9 kJ/mol
delta H(C02)=-393.5 kJ/mol
delta H(H20)=-241.8 kJ/mol

b) Determine the delta G standard state at 1000K. assume delta H is independent of temperature

Solution Preview

Use any good chemistry text reference. I'm using "Chemistry" 2nd ed. by Steven Zumdahl, page 749.

The free energy change is calculated using:
deltaG = deltaH - T*deltaS
Where ...

Solution Summary

The solution provides a detailed and step-by-step explanation for the problem.

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