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 

FREE Expert Solution
82% (127 ratings)
Problem Details

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

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.

How long does this problem take to solve?

Our expert Chemistry tutor, Sabrina took 8 minutes and 36 seconds to solve this problem. You can follow their steps in the video explanation above.