# Problem: Calcium carbonate can be converted to quick lime by the following reaction:CaCO3(s) → CaO(s) + CO2(g) Given that:       for CaCO3(s)  at 25°C     ΔHf° = -1206.9 kJ/mol  ΔS° = 92.9 J/mol K,                        for CaO(s)                     ΔHf° = -635.5 kJ/mol      ΔS° = 39.8 J/mol  K                        for CO2(g))                     ΔHf° = -393.5 kJ/mol     ΔS° = 213.6 J/mol  K Use these data to calculate ΔGo  for the reaction.A)  225.7 kJ/mole         B)   130.1 kJ/mole   C) -130.1 kJ/mole    D)    -225.7 kJ/mole      E)  none of these

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Calcium carbonate can be converted to quick lime by the following reaction:

CaCO3(s) → CaO(s) + CO2(g)

Given that:       for CaCO3(s)  at 25°C     ΔHf° = -1206.9 kJ/mol  ΔS° = 92.9 J/mol K,

for CaO(s)                     ΔHf° = -635.5 kJ/mol      ΔS° = 39.8 J/mol  K

for CO2(g))                     ΔHf° = -393.5 kJ/mol     ΔS° = 213.6 J/mol  K

Use these data to calculate ΔGo  for the reaction.

A)  225.7 kJ/mole         B)   130.1 kJ/mole   C) -130.1 kJ/mole    D)    -225.7 kJ/mole      E)  none of these