Exhibit 14-6 Consider the Reaction at Equilibrium Below and Its

Exhibit 14-6 Consider the reaction at equilibrium below and its corresponding equilibrium constant to answer the following question(s) .
2 NO₂ (g) 2 NO (g) + O₂(g) K p = 4.48*10^{- 13}
A pressure of 0.45 atm of NO₂ is introduced into a container and allowed to come to equilibrium.
Complete the ICE equilibrium table shown below to get started. Partial pressure S₂NO₂² NO O₂ Initial 0.45 M Change At equilibrium
-Refer to Exhibit 14-6. Using a simplifying assumption that x is small in any sums or differences, solve for x and determine what is the partial pressure of NO at equilibrium.

A) [NO]_eq = 2.8×10 ^{- 5} M
B) [NO]_eq = 3.6×10 ^{- 5} M
C) [NO]_eq = 3.7×10 ^{- 5} M
D) [NO]_eq = 5.7×10 ^{- 5} M
E) [NO]_eq = 7.4×10 ^{- 5} M