Nitrogen monoxide molecules can react to form dinitrogen oxide and nitrogen dioxide. Determine the equilibrium constant for this reaction under standard conditions from the following data and note whether the reaction is product-favored or reactant-favored.
$\Delta$ G^$\circ$(NO, g) = 86.6 kJ/mol
$\Delta$ G^$\circ$(N₂O, g) = 104.2 kJ/mol
$\Delta$ G^$\circ$(NO₂, g) = 51.3 kJ/mol

Question

Nitrogen monoxide molecules can react to form dinitrogen oxide and nitrogen dioxide. Determine the equilibrium constant for this reaction under standard conditions from the following data and note whether the reaction is product-favored or reactant-favored.

\Delta

G^$\circ$(NO, g) = 86.6 kJ/mol

\Delta

G^$\circ$(N₂O, g) = 104.2 kJ/mol

\Delta

G^$\circ$(NO₂, g) = 51.3 kJ/mol

Quizplus · Accepted Answer

The Answer of Nitrogen monoxide molecules can react to form dinitrogen oxide and nitrogen dioxide. Determine the equilibrium constant for this reaction under standard conditions from the following data and note whether the reaction is product-favored or reactant-favored. $\Delta$G $\circ$ (NO, g) = 86.6 kJ/mol $\Delta$G $\circ$ (N₂O, g) = 104.2 kJ/mol $\Delta$G $\circ$ (NO₂, g) = 51.3 kJ/mol

Nitrogen Monoxide Molecules Can React to Form Dinitrogen Oxide and Nitrogen