Question

For the reaction 2NO(g)+O₂(g) ⇌ 2NO₂(g) at a certain temperature, the equilibrium concentrations were found to be [NO₂]= 3.3 x 10⁻³ M, [ O₂ ] = 1.2 x 10⁻² M, and [NO] = 2.0 x 10⁻³ M. Calculate the value of the equilibrium constant from these data.

Answer 1

The equilibrium constant (Kc) for the reaction 2NO(g) + O2(g) ⇌ 2NO2(g) is calculated using the given equilibrium concentrations, yielding a value of 2.26 × 10¹.

Step-by-step explanation:

To calculate the equilibrium constant (Kc) for the reaction 2NO(g) + O2(g) ⇌ 2NO2(g) given the equilibrium concentrations, we use the expression:

Kc = [NO2]2 / ([NO]2 × [O2])

Substituting the given equilibrium concentrations, we have:

Kc = (3.3 × 10−3M)2 / ((2.0 × 10−3M)2 × 1.2 × 10−2M)

This gives us:

Kc = (10.89 × 10−6M2) / (4.0 × 10−6M2 × 1.2 × 10−2M)

So, Kc = 2.26 × 101

Therefore, the value of the equilibrium constant for this reaction at the given temperature is 2.26 × 101.