Use the data given here to calculate the values of ΔG° rxn at 25°C for the reaction described by the equation:
A+B >C
Compound A 387.7
Compound B -653.3
Compound C 402.0
a) Find ΔG Rxn in kj/mol.

The Gibbs free energy ΔG Rxn for the reaction A + B ⇄ C  is 667.6 kJ

The Standard Gibbs free energy is the rate at which the reactant is being changed to products. It can be expressed by using the formula:

Therefore, from the reaction between A + B ⇄ C, we can conclude that the  ΔG Rxn is 667.6 kJ

Learn more about ΔG° rxn here:

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For the following reaction ΔG°rxn = 667.6 kJ/mol

Explanation:

Step 1: Data given

Temperature = 25 °C

Compound A  = 387.7  kJ/mol

Compound B = -653.3  kJ/ mol

Compound C =  402.0 kJ/mol

Step 2: The balanced equation

A + B → C

Step 3: Find ΔG Rxn in kj/mol.

ΔG°rxn = ΔG°products - ΔG°reactants

ΔG°rxn = 402.0 kJ/mol - (387.7 kJ/mol -653.3 kJ/mol)

ΔG°rxn = 402.0 kJ/mol - (-265.6 kJ/mol)

ΔG°rxn = 402.0 kJ/mol + 265.6 kJ/mol

ΔG°rxn = 667.6 kJ/mol

For the following reaction ΔG°rxn = 667.6 kJ/mol

c

explanation: