Exhibit 17-4 Consider the reaction of nitrogen monoxide and oxygen gas to form nitrogen dioxide as shown below to answer the following question(s) . NO (g) + O₂ (g) →2 NO₂ (g)
-Refer to Exhibit 17-4. Given that D S ° _rxn = - 146.5 Jmol^{- 1}K^{- 1} and D H ° _rxn = - 114.2. kJ/mol for this reaction, what is the standard Gibbs Free Energy, D G ° _rxn, for this reaction at 500 K?

Question

Quizplus · Accepted Answer

The standard Gibbs free energy of reaction can be calculated using the equation: D G ° = D H ° - T D S ° Where D H ° and D S ° are the standard enthalpy and entropy changes, respectively, and T is the temperature in Kelvin. Substituting the given values, we get: D G ° = (−114.2 kJ/mol) − (500 K)(−146.5 J/mol K)/(1000 J/kJ) D G ° = −41.0 kJ/mol Therefore, the correct answer is B - D G ° _rxn= - 41.0 kJ/mol.

Exhibit 17-4 Consider the Reaction of Nitrogen Monoxide and Oxygen