For the equilibrium CO₂(g)+ N₂(g)$\leftrightarrows$ CO(g)+ N₂O(g),the forward and reverse rate constants at 1200 K are 9.1 $\times$ 10^-11 M ^-¹s^-¹ and 1.5 $\times$ 10⁵ M ^-¹s^-¹,respectively.What is the value of the equilibrium constant for CO(g)+ N₂O(g)$\leftrightarrows$ CO₂(g)+ N₂(g)?

Question

Quizplus · Accepted Answer

The equilibrium constant is the ratio of the forward and reverse rate constants. Therefore, the equilibrium constant for the given reaction is:K = (9.1 F1F1F1S1F1F1F10 10F1F1F1S1^F1F1F10¹¹ M ^-¹s^-¹) / (1.5 F1F1F1S1F1F1F10 10⁵ M ^-¹s^-¹) = 6.1 F1F1F1S1F1F1F10 10F1F1F1S1^F1F1F10¹⁶

For the Equilibrium CO2(g)+ N2(g) ⇆\leftrightarrows⇆ CO(g)+ N2O(g),the Forward and Reverse Rate Constants at 1200 K

For the Equilibrium CO₂(g)+ N₂(g) $\leftrightarrows$ CO(g)+ N₂O(g),the Forward and Reverse Rate Constants at 1200 K