Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 °C, K_c equals 1.0 × 10?⁵. N₂(g) + O₂(g) $\rightleftharpoons$ 2 NO(g)
If 0.030 mol N₂ and 0.030 mol O₂ are sealed in a 1.0 L flask at 1500 °C, what is the concentration of NO(g) when equilibrium is established?

Question

Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 °C, K_c equals 1.0 × 10?⁵. N₂(g) + O₂(g)

\rightleftharpoons

2 NO(g)
If 0.030 mol N₂ and 0.030 mol O₂ are sealed in a 1.0 L flask at 1500 °C, what is the concentration of NO(g) when equilibrium is established?

Quizplus · Accepted Answer

The equilibrium constant expression is Kc = [NO]^2 / ([N2][O2]). Given Kc = 1.0 × 10^-5 and initial concentrations [N2] = [O2] = 0.030 M, solving for [NO] at equilibrium gives approximately 9.5 × 10^-5 M.

Nitrogen and Oxygen Gases May React to Form Nitrogen Monoxide ⇌\rightleftharpoons⇌

Nitrogen and Oxygen Gases May React to Form Nitrogen Monoxide $\rightleftharpoons$