What is ΔGo at 1000 oC for the following reaction?
CaCO3 (s) CaO (s) + CO2 (g)
To find the value of ΔGo at 1000°C for the given reaction, we need to use the Gibbs free energy equation and the values of standard Gibbs free energy of formation for the reactants and products involved.
The Gibbs free energy change (ΔGo) can be calculated using the equation:
ΔGo = ΣΔGo(products) - ΣΔGo(reactants)
First, let's identify the standard Gibbs free energy of formation (∆Gof) values for the reactants and products. The ∆Gof values represent the change in Gibbs free energy when one mole of a compound is formed from its constituent elements in their standard states at a specific temperature and pressure.
The standard Gibbs free energy of formation values at 1000°C for the substances involved in the reaction are as follows:
∆Gof(CaCO3) = -1328.6 kJ/mol
∆Gof(CaO) = -604.4 kJ/mol
∆Gof(CO2) = -394.4 kJ/mol
Now, we can calculate ΔGo:
ΔGo = ∆Gof(CaO) + ∆Gof(CO2) - ∆Gof(CaCO3)
= -604.4 + (-394.4) - (-1328.6)
= -604.4 - 394.4 + 1328.6
= 329.8 kJ/mol
Therefore, ΔGo at 1000°C for the given reaction, CaCO3 (s) → CaO (s) + CO2 (g), is 329.8 kJ/mol.