Question

Nitrogen monoxide, NO, is formed in automobile exhaust by the reaction of nitrogen and oxygen in the air: N2 (g) + O2 (g) ↔ NO (g) BALANCE THE EQUATION The equilibrium constant Kc is 0.0025 at 2127 oC. If an equilibrium mixture at this temperature contains 0.023 M N2 and 0.031 M O2, what is the equilibrium concentration of NO? __________ M NO

Answer 1

The equilibrium concentration of nitrogen monoxide (NO) can be calculated by rearranging the equilibrium constant expression, inserting the known values, and solving for [NO].

Step-by-step explanation:

The balanced chemical equation for the formation of nitrogen monoxide (NO) in automobile exhaust, which is the reaction of nitrogen (N2) and oxygen (O2) gases, is: N2 (g) + O2 (g) ⇌ 2 NO (g).

The equilibrium constant expression for this reaction at a given temperature is Kc = [NO]2 / ([N2] × [O2]). Given that Kc = 0.0025 at 2127 °C, and the equilibrium concentrations of N2 and O2 are 0.023 M and 0.031 M respectively, we can set up an equation to solve for the equilibrium concentration of NO:

0.0025 = [NO]2 / (0.023 × 0.031)

To find [NO], we can solve for [NO]2 = 0.0025 × 0.023 × 0.031 and then find the square root of the result to obtain the equilibrium concentration of NO.

Answer 2

The equilibrium concentration of NO is 0.001335 M

Step-by-step explanation:

Step 1: Data given

The equilibrium constant Kc is 0.0025 at 2127 °C

An equilibrium mixture contains 0.023M N2 and 0.031 M O2,

Step 2: The balanced equation

N2(g) + O2(g) ↔ 2NO(g)

Step 3: Concentration at the equilibrium

[N2] = 0.023 M

[O2] = 0.031 M

Kc = 0.0025 = [NO]² / [N2][O2]

Kc = 0.0025 = [NO]² / (0.023)(0.031)

[NO] = 0.001335 M

The equilibrium concentration of NO is 0.001335 M