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.
Determine the equilibrium concentration for each of the substance
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.