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90. Consider this reaction occurring at 298 K: BaCO3(s) = BO(s) + CO2(g) a. Show that the reaction is not spontaneous under standard conditions by calculating AGrxn- b. If BaCO3 is placed in an evacuated flask, what is the partial pressure of CO2 when the reaction reaches equilibrium? c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, at what temperature is the partial pressure of carbon dioxide 1.0 atm?
90. Consider this reaction occurring at 298 K: BaCO3(s) = BO(s) + CO2(g) a. Show that the reaction is not spontaneous under standard conditions by calculating AGrxn- b. If BaCO3 is placed in an evacuated flask, what is the partial pressure of CO2 when the reaction reaches equilibrium? c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, at what temperature is the partial pressure of carbon dioxide 1.0 atm?
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Patrina SchowalterLv2
30 Mar 2018
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