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13 Dec 2019

Using Statistical Thermodynamic equations, calculate thefollowing thermodynamic properties: Energy, Enthalpy, GibbsFree-Energy, and Entropy for HI at standard pressure (1 atm) and 25degrees C. De=228kJ/mol

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Consider a combustion of butyric acid at , and the thermodynamic data provided:

Substance	Enthalpy, ,	Entropy, ,





	?

From the data above, calculate the standard heat formation, for butyric acid at

Calculate the standard free energy of formation for butyric acid at .

(Hint: Use the reaction to find and and use those to calculate . In this case,

amberjellyfish517

The thermodynamic properties for areaction are related by the equation that defines the standard freeenergy, ?G?, in kJ/mol:

?G?=?H??T?S?

where ?H? is the standard enthalpy changein kJ/moland ?S? is the standard entropy changein J/(mol?K). A good approximation of the free energychange at other temperatures, ?GT, can also beobtained by utilizing this equation and assuming enthalpy(?H?) and entropy (?S?) change little withtemperature.

****PartA

For the decomposition of calciumcarbonate, consider the following thermodynamic data:

?H?rxn	178.5kJ/mol
?S?rxn	161.0J/(mol?K)

Calculate the temperature in kelvins above which this reaction isspontaneous.

Express your answer to foursignificant figures and include the appropriate units.

The standard free energy change,?G?, and the equilibrium constantK for a reaction can be related by the followingequation:

?G?=?RTlnK

where T is the Kelvin temperature and R is equal to 8.314 J/(mol?K).

****PartB

Calculate the equilibrium constant forthe following reaction at room temperature, 25 ?C:

CaCO3(s)?CaO(s)+CO2(g)

Express your answernumerically to three significant figures.

****PART A (Unrelated)

The normalboiling point of Br2(l) is 58.8 ?C, andits molar enthalpy of vaporization is ?Hvap= 29.6 kJ/mol.

Calculatethe value of ?Swhen 1.70molof Br2(l) is vaporized at 58.8 ?C.

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Using Statistical Thermodynamic equations, calculate thefollowing thermodynamic properties: Energy, Enthalpy, GibbsFree-Energy, and Entropy for HI at standard pressure (1 atm) and 25degrees C. De=228kJ/mol

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