Calculate the change in Gibb’s free energy when 1.63 moles of sodium metal react with excess chlorine gas to form sodium chloride . Assume standard conditions. The ΔG values can be found in your textbook. The units for the answer are kJ

Isn't this the same as your previous two or three dG problems?

To calculate the change in Gibbs free energy (ΔG) for a given reaction, you'll need to utilize the standard Gibbs free energy change (ΔG°) values for the reactants and products. These values can typically be found in a chemistry textbook or online reference.

Here's how you can calculate the change in Gibbs free energy for the reaction between sodium (Na) and chlorine (Cl2) to form sodium chloride (NaCl):

1. Write the balanced chemical equation for the reaction:
2Na + Cl2 -> 2NaCl

2. Find the standard Gibbs free energy change (ΔG°) values for each component of the reaction.
The standard Gibbs free energy change values are typically provided in kilojoules per mole (kJ/mol).

- Look up the ΔG° value for sodium (Na). Let's assume its value is -50 kJ/mol.
- Look up the ΔG° value for chlorine (Cl2). Assume its value is -20 kJ/mol.
- Look up the ΔG° value for sodium chloride (NaCl). Let's assume its value is -150 kJ/mol.

3. Calculate the change in Gibbs free energy (ΔG) using the ΔG° values of the products and reactants.

ΔG = (n * ΔG°products) - (m * ΔG°reactants)

Where:
n = number of moles of products (NaCl)
m = number of moles of reactants (Na)

In this case, n = 1.63 moles (since sodium chloride is the only product)
m = 2 moles (since sodium appears as a reactant)

ΔG = (1.63 * -150) - (2 * -50)
= -244.5 kJ - (-100 kJ)
= -244.5 kJ + 100 kJ
= -144.5 kJ

Therefore, the change in Gibbs free energy (ΔG) for the reaction is approximately -144.5 kJ.