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18 Dec 2019

The standard Gibbs-free energy of a system is related to itsequilibrium constant through the following equation.

ΔG° = -R · T · ln(K)

In this equation R is the gas constant, T is the temperature, andthe ° next to ΔG defines the conditions as standard ambienttemperature and pressure, i.e. "SATP". (Answer the followingquestions to three significant figures.)

Suppose a reaction has a standard Gibbs-free energy of -13.9kJ/mol, calculate the relative ratio of product to reactant.

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Hubert Koch
Hubert KochLv2
31 Dec 2019

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Related questions

1) A reaction has ΔH∘rxn= -116 kJ and ΔS∘rxn= 324 J/K .

At what temperature is the change in entropy for the reaction equal to the change in entropy for the surroundings? Express your answer in kelvins.

2) Consider the following reaction:

2Ca(s)+O2(g) → 2CaO(s)

ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K

Assume that all reactants and products are in their standard states.

Calculate the free energy change for the reaction at 19 ∘C.

Express your answer using four significant figures.

3) Consider the following isomerization reactions of some simple sugars and values for their standard Gibbs free energy ΔG∘:

reaction
reaction A: glucose-1-phosphate⟶glucose-6-phosphate ΔG∘=−7.28 kJ/mol
reaction B: fructose-6-phosphate⟶glucose-6-phosphate, ΔG∘=−1.67 kJ/mol
Calculate ΔG∘ for the isomerization of glucose-1-phosphate to fructose-6-phosphate.
Express your answer with the appropriate units.

On a separate sheet of paper, draw the two alternative chair conformations for the product formed by the addition of bromine to 4-tert-butylcyclohexene. The Gibbs free-energy differences between equatorial and axial substituents on a cyclohexane ring are 21 kJ/mol for tert-butyl, and 2.3 kJ/mol for bromine. Calculate the ratio of the two observed products at 34.0 °C using the following equation: The gas constant, R, is 8.314 J/K·mol. (Enter your answer to two significant figures.)

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