Question

An equilibrium mixture of N2, O2and NO gases at 1500K is determined to consist of 6.4 x 10-3Mof N2, 1.7 x 10-3M O2, and 1.1 x 10-5M NO. Write the equilibrium expression and solve for the equilibrium constant (Keq) for the systemat this temperature?

Answer 1

The equilibrium constant (Keq) for the reaction N2(g) + O2(g) ⇌ 2NO(g) at 1500K is calculated using the equilibrium concentrations and is determined to be 1.19 x 10^-4.

Step-by-step explanation:

The student has presented an equilibrium scenario involving nitrogen (N₂), oxygen (O₂), and nitrogen monoxide (NO) at a temperature of 1500K. To determine the equilibrium constant (Keq) for the reaction N₂(g) + O₂(g) ⇌ 2NO(g), we can use the given equilibrium concentrations of N₂, O₂, and NO.

The equilibrium expression for the reaction is:

Keq = [NO]2 / ([N₂][O₂])

Inserting the equilibrium concentrations provided, we get:

Keq = (1.1 x 10^−5 M)2 / ((6.4 x 10^−3 M)(1.7 x 10^−3 M))

After calculating, we find:

Keq = 1.19 x 10^−4

This value is the equilibrium constant for the reaction at 1500K.

Answer 2

Explanation:O2 = 1.7×10-3M;

N2 = 6.4×10-3M;

NO = 1.1 10-5M.