Calculate G° for each reaction using G°f values.
MnO2(s) + 2 CO(g) Mn(s) + 2 CO2(g)
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To calculate ΔG° (standard Gibbs free energy change) for a reaction using the standard Gibbs free energy of formation (ΔG°f) values, you need to follow these steps:
1. Write the balanced equation for the reaction:
MnO2(s) + 2 CO(g) → Mn(s) + 2 CO2(g)
2. Look up the standard Gibbs free energy of formation (ΔG°f) values for each compound involved in the reaction. These values are tabulated and can be found in reference books or online databases. Here are the values for the given compounds:
ΔG°f(MnO2) = -588.7 kJ/mol
ΔG°f(CO) = -137.3 kJ/mol
ΔG°f(Mn) = 0 kJ/mol
ΔG°f(CO2) = -394.4 kJ/mol
3. Calculate the ΔG° for the reaction using the following formula:
ΔG° = ΣnΔG°f(products) - ΣmΔG°f(reactants)
Σn is the stoichiometric coefficient of the product/compound.
Σm is the stoichiometric coefficient of the reactant/compound.
Plugging the values from step 2 into the formula, we get:
ΔG° = (1 × 0 kJ/mol) + (2 × -394.4 kJ/mol) - (1 × -588.7 kJ/mol) - (2 × -137.3 kJ/mol)
4. Calculate the ΔG° using the values obtained in step 3:
ΔG° = -334.2 kJ/mol
Therefore, the standard Gibbs free energy change (ΔG°) for the given reaction is -334.2 kJ/mol.