In a chemical reaction,4 mol of nitrogen monoxide(NO) and 2.5mol of Oxygen(O2) are being mixed togethere in a container with a volume of 1L to produce Nitrogen dioxide (NO2).If the Kc(Equilibrium constant) for this reaction in 0.001.

Question

Determine the equilibrium concentration for each of the substance

Answer 1

Let's first write the balanced equation for the reaction:

2NO(g) + O2(g) ⇌ 2NO2(g)

We have 4 mol of NO and 2.5 mol of O2 initially, in a 1L container. This means that the initial concentration of NO is 4 mol/1L = 4 M, and the initial concentration of O2 is 2.5 mol/1L = 2.5 M. The initial concentration of NO2 is 0 M.

Let's assume that x mol/L of NO is consumed and O2 is consumed in the reaction. This should be equal to twice the amount of NO2 produced, as per the balanced equation.

After the reaction reaches equilibrium, we have:
[NO] = 4 - x M
[O2] = 2.5 - x M
[NO2] = 0 + 2x M

Now, we can plug these values into the equilibrium expression for Kc:

Kc = [NO2]^2 / ([NO] * [O2])

0.001 = (2x)^2 / ((4-x)(2.5-x))

Solving this equation will give us the equilibrium concentration for each of the substances. This is a quadratic equation, and solving it requires calculating x first. Once we have the value of x, we can plug it back into the above expressions to find the equilibrium concentrations.