Answer:
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
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:
[tex]\mathbf{\Delta G^0_{rxn} = \sum (product) - \sum (reactant)}[/tex]
[tex]\mathbf{\Delta G^0_{rxn} =(1 \times 402) -((1 \times 387.7)+ (1 \times -653.3) )}[/tex]
[tex]\mathbf{\Delta G^0_{rxn} =(402 - 387.7+ 653.3 ) \ kJ}[/tex]
[tex]\mathbf{\Delta G^0_{rxn} =667.6\ kJ}[/tex]
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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