What is ΔG°_rxnfor the following reaction? 2NO(g) + Cl₂(g) → 2NOCl(g) A) -40.40 kJ/mol B) +40.40 kJ/mol C) -20.20 kJ/mol D) +20.20 kJ/mol E) +152.90 kJ/mol

Question

Quizplus · Accepted Answer

To calculate ΔG° for the reaction, we need to use standard Gibbs free energy of formation (ΔG°f) values for the reactants and products.

Using these values, we can calculate the standard Gibbs free energy change (ΔG°) for the reaction using the equation: 
ΔG°rxn = ΣnΔG°f(products) - ΣnΔG°f(reactants)

Given ΔG°f values: 
NO(g) = 86.7 kJ/mol 
Cl2(g) = 0 kJ/mol 
NOCl(g) = 51.8 kJ/mol

ΔG°rxn = (2 mol)(51.8 kJ/mol) - [ (2 mol)(86.7 kJ/mol) + (1 mol)(0 kJ/mol) ] 
ΔG°rxn = -40.4 kJ/mol

Therefore, the answer is A) -40.40 kJ/mol.

What Is ΔG°rxn for the Following Reaction? 2NO(g) + Cl2(g)

What Is ΔG°_rxnfor the Following Reaction? 2NO(g) + Cl₂(g)