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Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Calculate the temperature in kelvins above which this reaction is spontaneous.

Express your answer to four significant figures and include the appropriate units.
<Hw8-Chapter19 + Gibbs Free Energy: Equilibrium Constant 10 of 17 : I Review | Constants | Periodic Table Calcium oxide, CaO, is manufactured by decomposition of calcium carbonate, CaCO3. in a furnace at 500 K: Relation among thermodynamic quantities CaCO, (s)->CaO(s) + CO2(g) The thermodynamic properties for a reaction are related by the equation that defines the standard free energy. AG", in kJ/mol: The spontaneity of a reaction can be determined from the free energy change for the reaction, AG AG" ΔΗ' TAS • A reaction is spontaneous when the free energy change is less than zero. • A reaction is nonspontaneous when the free energy change is greater than zero. • A reaction is in equilibrium when the free energy change is equal to zero. where AH® is the standard enthalpy change in kJ/mol and AS° is the standard entropy change in J/(mol - K). A good approximation of the free energy change at other temperatures, AGT. can also be obtained by utilizing this equation and assuming enthalpy (AH°) and entropy (AS®) change little with temperature. Part A For the decomposition of calcium carbonate, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer.): | ΔΗ 178.5kJ/mol ASan 161.0J/(mol - K) 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) HA T = Value Units Submit
Transcribed Image Text:<Hw8-Chapter19 + Gibbs Free Energy: Equilibrium Constant 10 of 17 : I Review | Constants | Periodic Table Calcium oxide, CaO, is manufactured by decomposition of calcium carbonate, CaCO3. in a furnace at 500 K: Relation among thermodynamic quantities CaCO, (s)->CaO(s) + CO2(g) The thermodynamic properties for a reaction are related by the equation that defines the standard free energy. AG", in kJ/mol: The spontaneity of a reaction can be determined from the free energy change for the reaction, AG AG" ΔΗ' TAS • A reaction is spontaneous when the free energy change is less than zero. • A reaction is nonspontaneous when the free energy change is greater than zero. • A reaction is in equilibrium when the free energy change is equal to zero. where AH® is the standard enthalpy change in kJ/mol and AS° is the standard entropy change in J/(mol - K). A good approximation of the free energy change at other temperatures, AGT. can also be obtained by utilizing this equation and assuming enthalpy (AH°) and entropy (AS®) change little with temperature. Part A For the decomposition of calcium carbonate, consider the following thermodynamic data (Due to variations in thermodynamic values for different sources, be sure to use the given values in calculating your answer.): | ΔΗ 178.5kJ/mol ASan 161.0J/(mol - K) 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) HA T = Value Units Submit
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