Consider the equilibrium 2 NO(g)$\leftrightarrows$ N₂(g)+ O₂(g).At 1400 K,the equilibrium constant is approximately 2.6 $\times$ 10⁵.What is true about this equilibrium?

Question

Quizplus · Accepted Answer

The equilibrium constant (K) is a value that represents the ratio of the forward and reverse reaction rates at equilibrium. In this equation, the value of K is given as 2.6 x 10^10, indicating that the forward reaction rate (k_forward) is much larger than the reverse reaction rate (k_reverse), as K = k_forward/k_reverse. Therefore, choice D is correct. Choices A, B, and E are incorrect because they make assumptions or statements that are not supported by the given information. Choice C is incorrect because K is not equal to 1.

Consider the Equilibrium 2 NO(g) ⇆\leftrightarrows⇆ N2(g)+ O2(g) ×\times× 105

Consider the Equilibrium 2 NO(g) $\leftrightarrows$ N₂(g)+ O₂(g) $\times$ 10⁵