In the atmosphere, nitrogen gas can react with ozone (O₃) to form nitrogen dioxide and oxygen gas.Write the balanced reaction equilibrium using the smallest whole-number coefficients possible.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.
$\Delta G^{\circ}\left(\mathrm{O}_{3}, g\right)=163.2 \mathrm{~kJ} / \mathrm{mol}$
$\Delta G^{\circ}\left(\mathrm{NO}_{2}, g\right)=51.3 \mathrm{~kJ} / \mathrm{mol}$

Question

In the atmosphere, nitrogen gas can react with ozone (O₃) to form nitrogen dioxide and oxygen gas.Write the balanced reaction equilibrium using the smallest whole-number coefficients possible.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}\left(\mathrm{O}_{3}, g\right)=163.2 \mathrm{~kJ} / \mathrm{mol}

\Delta G^{\circ}\left(\mathrm{NO}_{2}, g\right)=51.3 \mathrm{~kJ} / \mathrm{mol}

Quizplus · Accepted Answer

The Answer of In the atmosphere, nitrogen gas can react with ozone (O₃) to form nitrogen dioxide and oxygen gas.Write the balanced reaction equilibrium using the smallest whole-number coefficients possible.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}\left(\mathrm{O}_{3}, g\right)=163.2 \mathrm{~kJ} / \mathrm{mol} $ $ \Delta G^{\circ}\left(\mathrm{NO}_{2}, g\right)=51.3 \mathrm{~kJ} / \mathrm{mol} $

In the Atmosphere, Nitrogen Gas Can React with Ozone (O3) ΔG∘(O3,g)=163.2 kJ/mol \Delta G^{\circ}\left(\mathrm{O}_{3}, g\right)=163.2 \mathrm{~kJ} / \mathrm{mol} ΔG∘(O3​,g)=163.2 kJ/mol

In the Atmosphere, Nitrogen Gas Can React with Ozone (O₃) $\Delta G^{\circ}\left(\mathrm{O}_{3}, g\right)=163.2 \mathrm{~kJ} / \mathrm{mol}$