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Consider the reaction shown below. Calculate the equilibrium pressure of CO₂ in the system at the following temperatures. (a) 290°C (b).480°C. Xatm xatm PbCO3(s) = PbO(s) + CO₂(g) Note: To find the value of the equilibrium constant at each temperature you must first find the value of AGO at each temperature by using the equation AGO=AHⓇ - TASO For this reaction the values are AH° +88.3 kJ/mol and AS°= 151.3 J/mol K

Consider the reaction shown below. Calculate the equilibrium pressure of CO₂ in the system at the following temperatures. (a) 290°C (b).480°C. Xatm xatm PbCO3(s) = PbO(s) + CO₂(g) Note: To find the value of the equilibrium constant at each temperature you must first find the value of AGO at each temperature by using the equation AGO=AHⓇ - TASO For this reaction the values are AH° +88.3 kJ/mol and AS°= 151.3 J/mol K

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.18PAE: The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures...
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Consider the reaction shown below. Calculate the equilibrium pressure of CO₂ in the system at the following temperatures. (a) 290°C (b) 480°C. X atm atm PbCO3(s) = PbO(s) + CO₂(g) Note: To find the value of the equilibrium constant at each temperature you must first find the value of AGO at each temperature by using the equation ΔGO = ΔΗΟ - ΤΔ0 For this reaction the values are AHO = +88.3 kJ/mol and AS⁰= 151.3 J/mol*K
Transcribed Image Text:Consider the reaction shown below. Calculate the equilibrium pressure of CO₂ in the system at the following temperatures. (a) 290°C (b) 480°C. X atm atm PbCO3(s) = PbO(s) + CO₂(g) Note: To find the value of the equilibrium constant at each temperature you must first find the value of AGO at each temperature by using the equation ΔGO = ΔΗΟ - ΤΔ0 For this reaction the values are AHO = +88.3 kJ/mol and AS⁰= 151.3 J/mol*K
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