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Free energy change of a reaction

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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.

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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 T ...

Solution Summary

The solution provides a detailed and step-by-step explanation that discusses the free energy change of a reaction.

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Calculating the Equilibrium Constant: Change in Free Energy

Survey of physical chemistry

State all of the assumptions (e.g. ideal gas etc).

(previous reaction is 2H??2(g) + O2(g) ----> 2H2O(g))

Given the reaction in the previous question at 298 Kelvin where H2 has a partial pressure of 0.10 bar, O2 is at 0.20 bar, and H2o is at 1.5 bar:
(a) Determine the direction and quantify the change in free energy the reaction must undergo to reach equilibrium.

(b) Calculate the equilibrium constant.

(c) Illustrate the reaction on a plot of Free Energy versus % Reactants/Products (show ?GO, the approximate position of Q for the given partial pressures, and the position of Q at equilibrium).

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