There are many reactions involving nitrogen,oxygen,and nitrogen oxides at high temperatures.At 1000.0 K,the following reactions have the given equilibrium constants: N₂O₄(g)$\leftrightarrows$ 2 NO₂(g)K₁ = 1.5 $\times$ 10⁶ N₂(g)+ O₂(g)$\leftrightarrows$ NO₂(g)K₂ = 1.2 $\times$10^-5 Calculate the theoretical value of the equilibrium constant for N₂(g)+ 2 O₂(g)$\leftrightarrows$ N₂O₄(g).

Question

Quizplus · Accepted Answer

The equilibrium constant for the reaction N₂(g)+ 2 O₂(g)F3S3S3W1F1F1F10 N₂O₄(g) can be calculated using the equilibrium constants of the two given reactions: N₂(g)+ O₂(g)F3S3S3W1F1F1F10 NO₂(g) We can use the equilibrium constant of this reaction to calculate the equilibrium constant of the desired reaction: K1 = [NO₂(g)] / [N₂(g)][O₂(g)] K desired = [N₂O₄(g)] / ([N₂(g)] [O₂(g)]^2) K desired = K1 * K₁ / K₂^(2) K desired = 1.5 * 10^(-10) / (1.2^2) K desired = 9.6 * 10^(-10)

There Are Many Reactions Involving Nitrogen,oxygen,and Nitrogen Oxides at High ⇆\leftrightarrows⇆

There Are Many Reactions Involving Nitrogen,oxygen,and Nitrogen Oxides at High $\leftrightarrows$