The thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C BaCO3(s)→BaO(s)+CO2(g)
The thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C BaCO3(s)→BaO(s)+CO2(g)
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter10: Entropy And The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 10.91PAE: The reaction shown below is involved in the refining of iron. (The table that follows provides all...
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The
| ΔH∘rxn | 243.5kJ/mol |
| ΔS∘rxn | 172.0J/(mol⋅K) |
Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C
BaCO3(s)→BaO(s)+CO2(g)
Transcribed Image Text:The following equation can be used to calculate AGº for this reaction:
ΔG ΔΗ-ΤΔS
What is the standard free energy change, AG°, in joules per mole for this
reaction?
Express your answer with the appropriate units.
• View Available Hint(s)
J
AG° = 1.92x105
mol
AG° :
%3D
Transcribed Image Text:For the decomposition of barium carbonate, consider the following thermodynamic data
(Due to variations in thermodynamic values for different sources,
values in calculating your answer.):
be sure to use the given
AHm
243.5kJ/mol
ASPn 172.0J/(mol · K)
xn.
Calculate the temperature in kelvins above which this reaction is spontaneous.
Express your answer to four significant figures and include the appropriate units.
• View Available Hint(s)
T = 1416 K
%3D
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