Given the following: I.N₂O(g)+ 1/2 O₂(g)⇌ 2 NO(g)K_c = 1.7 × 10^-13 II.N₂(g)+ O₂(g)⇌ 2 NO(g)K_c = 4.1 × 10^-31 Find the value of the equilibrium constant for the following equilibrium reaction: N₂(g)+ 1/2 O₂(g)⇌ N₂O(g) A)7.0 × 10^-44 B)4.2 × 10¹⁷ C)2.4 × 10^-18 D)1.6 × 10^-9 E)2.6 × 10^-22

Question

Quizplus · Accepted Answer

We can calculate the equilibrium constant for the given reaction by multiplying the equilibrium constants of the two given reactions. 
Kc = (Kc1/2) * (Kc2)
Kc = (1.7 × 10^-13 / 2) * (4.1 × 10^-31)
Kc = 2.4 × 10^-18
Therefore, the correct answer is C.

Given the Following: I.N2O(g)+ 1/2 O2(g)⇌ 2 NO(g)Kc = 1.7 × 10-13

Given the Following: I.N₂O(g)+ 1/2 O₂(g)⇌ 2 NO(g)K_c = 1.7 × 10^-13