The equilibrium constant (kp) for the formation of the air pollutant nitric oxide (no) in an automobile engine at 537°c is 4.5 × 10−11. n2(g) + o2(g) ⇌ 2no(g) (a) calculate the partial pressure of no under these conditions if the partial pressures of nitrogen and oxygen are 3.00 and 0.012 atm, respectively.

1.3 × 10⁻⁶ atm

Explanation:

Let's consider the following reaction at equilibrium.

N₂(g) + O₂(g) ⇄ 2 NO(g)

The equilibrium constant (Kp) is:

Given pN₂ = 3.00 atm and pO₂ = 0.012 atm, the partial pressure of NO is:

pNO² = Kp × pN₂ × pO₂ = 4.5 × 10⁻¹¹ × 3.00 × 0.012

pNO = 1.3 × 10⁻⁶ atm

in the analysis of systems that involve fluid flow, we frequently encounter the combination of properties u and pv.