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 1000ml 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

The balanced chemical equation for the reaction is:

2NO(g) + O2(g) -> 2NO2(g)

Given that 4 mol of NO and 2.5 mol of O2 are being mixed together in a container with a volume of 1000 ml, we can first calculate the initial concentrations of each species:

- Initial [NO] = 4 mol / 1000 ml = 0.004 mol/ml
- Initial [O2] = 2.5 mol / 1000 ml = 0.0025 mol/ml
- Initial [NO2] = 0 mol / 1000 ml = 0 mol/ml

Since the stoichiometry of the reaction is 2:1:2 for NO:O2:NO2, the change in concentration for each species can be represented by -2x, -x, and +2x respectively. Let x be the change in concentration.

Therefore, at equilibrium:
[NO] = 0.004 - 2x mol/ml
[O2] = 0.0025 - x mol/ml
[NO2] = 2x mol/ml

Given that the equilibrium constant Kc = [NO2]^2 / ([NO]^2 * [O2]), and Kc = 0.001, we can substitute the equilibrium concentrations into the expression for Kc and solve for x.

0.001 = (2x)^2 / ((0.004 - 2x)^2 * (0.0025 - x))

Solving this equation will give you the value of x, which in turn can be used to determine the equilibrium concentrations of NO, O2, and NO2.