Calculate the Delta G(not) for the reaction:

C(s) + CO2 (g) --> 2 CO

Delta Gf : CO2 = -394.4 kj/mol
Delta Gf : CO = -137.2 kj/mol

To calculate the standard Gibbs free energy change (ΔG°) for the reaction, you need to use the formula:

ΔG° = ΣnΔGf°(products) - ΣmΔGf°(reactants)

Where:
- ΣnΔGf°(products) represents the sum of the ΔGf° values for the products, multiplied by their coefficients.
- ΣmΔGf°(reactants) represents the sum of the ΔGf° values for the reactants, multiplied by their coefficients.

In this case, the reaction equation is:

C(s) + CO2(g) → 2CO

The ΔGf° values for the reactants and products are given as:

ΔGf°(CO2) = -394.4 kJ/mol
ΔGf°(CO) = -137.2 kJ/mol

Substituting these values into the formula, we have:

ΔG° = (2 * ΔGf°(CO)) - (ΔGf°(C) + ΔGf°(CO2))

ΔG° = (2 * -137.2 kJ/mol) - (0 + -394.4 kJ/mol)

Simplifying the expression, we get:

ΔG° = -274.4 kJ/mol + 394.4 kJ/mol

ΔG° = 120 kJ/mol

Therefore, the standard Gibbs free energy change (ΔG°) for the reaction C(s) + CO2(g) → 2CO is 120 kJ/mol.

To calculate the standard Gibbs free energy change (ΔG°) for a reaction, you need to use the standard Gibbs free energy of formation (ΔGf°) values for the reactants and products. The ΔGf° values represent the Gibbs free energy change when one mole of a compound is formed from its constituent elements, under standard conditions (which include a pressure of 1 atm and a temperature of 298 K).

Given the ΔGf° values for CO2 and CO, we can calculate the ΔG° for the given reaction as follows:

ΔG° = (n × ΔGf° products) - (m × ΔGf° reactants)

In this reaction, the reactants are C(s) and CO2(g), and the product is 2CO. The stoichiometric coefficients n and m indicate the number of moles of products and reactants, respectively.

So for the given reaction: CO2(g) + C(s) → 2CO

n = 2 (moles of CO)
m = 1 (moles of CO2)

ΔG° = (2 × ΔGf° CO) - (1 × ΔGf° CO2)

Substituting the given ΔGf° values:

ΔG° = (2 × (-137.2 kJ/mol)) - (1 × (-394.4 kJ/mol))

Calculating the values:

ΔG° = -274.4 kJ/mol + 394.4 kJ/mol

ΔG° = 120 kJ/mol

Therefore, the standard Gibbs free energy change (ΔG°) for the reaction C(s) + CO2(g) → 2CO is 120 kJ/mol.