Consider the following reaction: CaCO 3(s) <----> CaO (s) +CO 2 Using Thermodyna

Question

Consider the following reaction: CaCO3(s) <----> CaO(s) +CO2 Using Thermodynamic data tables calculate the equilibriumpressure of CO2 at 298K and 800K (Go CaCO3 = -1128.8 KJ/mol,Go CaO = -603.5 KJ/mol, GoCO2 = -394.4 KJ/mol) Consider the following reaction: CaCO3(s) <----> CaO(s) +CO2 Using Thermodynamic data tables calculate the equilibriumpressure of CO2 at 298K and 800K (Go CaCO3 = -1128.8 KJ/mol,Go CaO = -603.5 KJ/mol, GoCO2 = -394.4 KJ/mol) Using Thermodynamic data tables calculate the equilibriumpressure of CO2 at 298K and 800K (Go CaCO3 = -1128.8 KJ/mol,Go CaO = -603.5 KJ/mol, GoCO2 = -394.4 KJ/mol)

Explanation / Answer

CaCO3(s) <----> CaO(s) +CO2    : G G = G products - Greactants       = G CaO +G CO2 - G CaCO3       = -603.5 -394.4 -(-1128.8) KJ /mol          = +130.9 KJ / mol We know that G = - RT ln Kp      Where R = gas constant = 8.314 J/ mol - K                 T = Temperature = 298 K                 Kp = Equilibrium constant = ? So lnKp = - G / RT              = - 0.0528          Kp = 10^-0.0528               = 0.8854 From the Equation Kp = p CO2 * p CaO / pCaCO3        Since the partialpressures of solids are taken as unity  p CaO= p CaCO3 = 1 So p CO2 = 0.8854 Pa Simillarly the  p CO2 at 800K        Since the partialpressures of solids are taken as unity  p CaO= p CaCO3 = 1 So p CO2 = 0.8854 Pa Simillarly the  p CO2 at 800K

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